Topic 6: Chemical kinetics

Outline how a catalyst increases the rate of reaction.

Outline how a catalyst increases the rate of reaction.

Outline how a catalyst increases the rate of reaction.

Outline how a catalyst increases the rate of reaction.

Outline how a catalyst increases the rate of reaction.

Outline how a catalyst increases the rate of reaction.

Nitrogen monoxide reacts with oxygen gas to form nitrogen dioxide.

The following experimental data was obtained.

Deduce the partial order of reaction with respect to nitrogen monoxide and oxygen.

Nitrogen monoxide reacts with oxygen gas to form nitrogen dioxide.

The following experimental data was obtained.

Deduce the partial order of reaction with respect to nitrogen monoxide and oxygen.

Nitrogen monoxide reacts with oxygen gas to form nitrogen dioxide.

The following experimental data was obtained.

Deduce the partial order of reaction with respect to nitrogen monoxide and oxygen.

Which change causes the greatest increase in the initial rate of reaction between nitric acid and magnesium?

2HNO₃(aq) + Mg (s) → Mg(NO₃)₂ (aq) + H₂(g)

Which change causes the greatest increase in the initial rate of reaction between nitric acid and magnesium?

2HNO₃(aq) + Mg (s) → Mg(NO₃)₂ (aq) + H₂(g)

The diagram shows the Maxwell-Boltzmann curve for the uncatalyzed reaction.

Draw a distribution curve at a lower temperature (T₂) and show on the diagram how the addition of a catalyst enables the reaction to take place more rapidly than at T₁.

The diagram shows the Maxwell-Boltzmann curve for the uncatalyzed reaction.

Draw a distribution curve at a lower temperature (T₂) and show on the diagram how the addition of a catalyst enables the reaction to take place more rapidly than at T₁.

The diagram shows the Maxwell-Boltzmann curve for the uncatalyzed reaction.

Draw a distribution curve at a lower temperature (T₂) and show on the diagram how the addition of a catalyst enables the reaction to take place more rapidly than at T₁.

Outline two ways in which the progress of the reaction can be monitored. No practical details are required.

Outline two ways in which the progress of the reaction can be monitored. No practical details are required.

Outline two ways in which the progress of the reaction can be monitored. No practical details are required.

Suggest the relationship that points A, B and C show between the concentration of the acid and the rate of reaction.

Suggest the relationship that points A, B and C show between the concentration of the acid and the rate of reaction.

Suggest the relationship that points A, B and C show between the concentration of the acid and the rate of reaction.

Which change increases the rate of formation of hydrogen when zinc reacts with excess hydrochloric acid, assuming all other conditions remain the same?

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

A.     Adding water to the hydrochloric acid

B.     Decreasing the temperature

C.     Increasing the volume of hydrochloric acid

D.     Decreasing the size of the zinc particles while keeping the total mass of zinc the same

Which change increases the rate of formation of hydrogen when zinc reacts with excess hydrochloric acid, assuming all other conditions remain the same?

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

A.     Adding water to the hydrochloric acid

B.     Decreasing the temperature

C.     Increasing the volume of hydrochloric acid

D.     Decreasing the size of the zinc particles while keeping the total mass of zinc the same

Outline two ways in which the progress of the reaction can be monitored. No practical details are required.

Outline two ways in which the progress of the reaction can be monitored. No practical details are required.

Outline two ways in which the progress of the reaction can be monitored. No practical details are required.

Suggest the relationship that points A, B and C show between the concentration of the acid and the rate of reaction.

Suggest the relationship that points A, B and C show between the concentration of the acid and the rate of reaction.

Suggest the relationship that points A, B and C show between the concentration of the acid and the rate of reaction.

Suggest why there is a small increase in the surface pressure as the area is reduced to about 240 cm², but a much faster increase when it is further reduced.

Suggest why there is a small increase in the surface pressure as the area is reduced to about 240 cm², but a much faster increase when it is further reduced.

Suggest why there is a small increase in the surface pressure as the area is reduced to about 240 cm², but a much faster increase when it is further reduced.

Neither method actually gives the initial rate. Outline a method that would allow the initial rate to be determined.

Neither method actually gives the initial rate. Outline a method that would allow the initial rate to be determined.

Neither method actually gives the initial rate. Outline a method that would allow the initial rate to be determined.

The potential energy profile for the reversible reaction, X + Y ƒ$\rightleftharpoons$ Z is shown.

Which arrow represents the activation energy for the reverse reaction, Z → X + Y, with a catalyst?

The potential energy profile for the reversible reaction, X + Y ƒ$\rightleftharpoons$ Z is shown.

Which arrow represents the activation energy for the reverse reaction, Z → X + Y, with a catalyst?

Sketch a curve on the graph to show the volume of gas produced over time if the same mass of crushed calcium carbonate is used instead of lumps. All other conditions remain constant.

Sketch a curve on the graph to show the volume of gas produced over time if the same mass of crushed calcium carbonate is used instead of lumps. All other conditions remain constant.

Sketch a curve on the graph to show the volume of gas produced over time if the same mass of crushed calcium carbonate is used instead of lumps. All other conditions remain constant.

Which instrument would best monitor the rate of this reaction?

2KI (aq) + Cl₂(aq) → 2KCl (aq) + I₂(aq)

A.  Balance

B.  Colorimeter

C.  Volumetric flask

D.  Gas syringe

Which instrument would best monitor the rate of this reaction?

2KI (aq) + Cl₂(aq) → 2KCl (aq) + I₂(aq)

A.  Balance

B.  Colorimeter

C.  Volumetric flask

D.  Gas syringe

A student was investigating rates of reaction. In which of the following cases would a colorimeter show a change in absorbance?

A.  KBr (aq) + Cl₂(aq)

B.  Cu (s) + Na₂SO₄(aq)

C.  HCl (aq) + NaOH (aq)

D.  (CH₃)₃COH (aq) + K₂Cr₂O₇(aq)

A student was investigating rates of reaction. In which of the following cases would a colorimeter show a change in absorbance?

A.  KBr (aq) + Cl₂(aq)

B.  Cu (s) + Na₂SO₄(aq)

C.  HCl (aq) + NaOH (aq)

D.  (CH₃)₃COH (aq) + K₂Cr₂O₇(aq)

Sketch a graph of the concentration of iron(II) sulfate, FeSO₄, against time as the reaction proceeds.

Sketch a graph of the concentration of iron(II) sulfate, FeSO₄, against time as the reaction proceeds.

Sketch a graph of the concentration of iron(II) sulfate, FeSO₄, against time as the reaction proceeds.

Sketch a graph of the concentration of iron(II) sulfate, FeSO₄, against time as the reaction proceeds.

Sketch a graph of the concentration of iron(II) sulfate, FeSO₄, against time as the reaction proceeds.

Sketch a graph of the concentration of iron(II) sulfate, FeSO₄, against time as the reaction proceeds.

Outline, giving a reason, the effect of a catalyst on a reaction.

Outline, giving a reason, the effect of a catalyst on a reaction.

Outline, giving a reason, the effect of a catalyst on a reaction.

On the axes, sketch Maxwell–Boltzmann energy distribution curves for the reacting species at two temperatures T₁ and T₂, where T₂ > T₁.

On the axes, sketch Maxwell–Boltzmann energy distribution curves for the reacting species at two temperatures T₁ and T₂, where T₂ > T₁.

On the axes, sketch Maxwell–Boltzmann energy distribution curves for the reacting species at two temperatures T₁ and T₂, where T₂ > T₁.

Additional experiments were carried out at an elevated temperature. On the axes below, sketch Maxwell–Boltzmann energy distribution curves at two temperatures T₁ and T₂, where T₂ > T₁.

Additional experiments were carried out at an elevated temperature. On the axes below, sketch Maxwell–Boltzmann energy distribution curves at two temperatures T₁ and T₂, where T₂ > T₁.

Additional experiments were carried out at an elevated temperature. On the axes below, sketch Maxwell–Boltzmann energy distribution curves at two temperatures T₁ and T₂, where T₂ > T₁.

The graph below shows the Maxwell–Boltzmann distribution of molecular energies at a particular temperature.

The rate at which dinitrogen monoxide decomposes is significantly increased by a metal oxide catalyst.

Annotate and use the graph to outline why a catalyst has this effect.

The graph below shows the Maxwell–Boltzmann distribution of molecular energies at a particular temperature.

The rate at which dinitrogen monoxide decomposes is significantly increased by a metal oxide catalyst.

Annotate and use the graph to outline why a catalyst has this effect.

The graph below shows the Maxwell–Boltzmann distribution of molecular energies at a particular temperature.

The rate at which dinitrogen monoxide decomposes is significantly increased by a metal oxide catalyst.

Annotate and use the graph to outline why a catalyst has this effect.

Examine, giving a reason, whether the rate of lead dissolving increases with acidity at 18 °C.

Examine, giving a reason, whether the rate of lead dissolving increases with acidity at 18 °C.

Examine, giving a reason, whether the rate of lead dissolving increases with acidity at 18 °C.

Determine from the graph the rate of reaction at 20 s, in cm³ s⁻¹, showing your working.

Determine from the graph the rate of reaction at 20 s, in cm³ s⁻¹, showing your working.

Determine from the graph the rate of reaction at 20 s, in cm³ s⁻¹, showing your working.

Which properties can be monitored to determine the rate of the reaction?

Fe (s) + CuSO₄ (aq) → Cu (s) + FeSO₄ (aq)

    I. change in volume
    II. change in temperature
    III. change in colour

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Which properties can be monitored to determine the rate of the reaction?

Fe (s) + CuSO₄ (aq) → Cu (s) + FeSO₄ (aq)

    I. change in volume
    II. change in temperature
    III. change in colour

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Examine, giving a reason, whether the rate of lead dissolving increases with acidity at 18 °C.

Examine, giving a reason, whether the rate of lead dissolving increases with acidity at 18 °C.

Examine, giving a reason, whether the rate of lead dissolving increases with acidity at 18 °C.

Which properties can be monitored to determine the rate of the reaction?

Fe (s) + CuSO₄ (aq) → Cu (s) + FeSO₄ (aq)

    I. change in volume
    II. change in temperature
    III. change in colour

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Which properties can be monitored to determine the rate of the reaction?

Fe (s) + CuSO₄ (aq) → Cu (s) + FeSO₄ (aq)

    I. change in volume
    II. change in temperature
    III. change in colour

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

Explain how the catalyst increases the rate of the reaction.

Explain how the catalyst increases the rate of the reaction.

Explain how the catalyst increases the rate of the reaction.

Explain how the catalyst increases the rate of the reaction.

Explain how the catalyst increases the rate of the reaction.

Explain how the catalyst increases the rate of the reaction.

Explain, referring to the Maxwell–Boltzmann distribution curve, the effect of a catalyst on a chemical reaction.

Explain, referring to the Maxwell–Boltzmann distribution curve, the effect of a catalyst on a chemical reaction.

Explain, referring to the Maxwell–Boltzmann distribution curve, the effect of a catalyst on a chemical reaction.

Annotate the Maxwell–Boltzmann distribution curve showing the activation energies, E_a, for the catalysed and uncatalysed reactions.

Annotate the Maxwell–Boltzmann distribution curve showing the activation energies, E_a, for the catalysed and uncatalysed reactions.

Annotate the Maxwell–Boltzmann distribution curve showing the activation energies, E_a, for the catalysed and uncatalysed reactions.

Sodium thiosulfate reacts with hydrochloric acid as shown:

Na₂S₂O₃ (aq) + 2HCl (aq) → S (s) + SO₂ (aq) + 2NaCl (aq) + H₂O (l)

The precipitate of sulfur makes the mixture cloudy, so a mark underneath the reaction mixture becomes invisible with time.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Sodium thiosulfate reacts with hydrochloric acid as shown:

Na₂S₂O₃ (aq) + 2HCl (aq) → S (s) + SO₂ (aq) + 2NaCl (aq) + H₂O (l)

The precipitate of sulfur makes the mixture cloudy, so a mark underneath the reaction mixture becomes invisible with time.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Sodium thiosulfate reacts with hydrochloric acid as shown:

Na₂S₂O₃ (aq) + 2HCl (aq) → S (s) + SO₂ (aq) + 2NaCl (aq) + H₂O (l)

The precipitate of sulfur makes the mixture cloudy, so a mark underneath the reaction mixture becomes invisible with time.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Explain, referring to the Maxwell–Boltzmann distribution curve, the effect of a catalyst on a chemical reaction.

Explain, referring to the Maxwell–Boltzmann distribution curve, the effect of a catalyst on a chemical reaction.

Explain, referring to the Maxwell–Boltzmann distribution curve, the effect of a catalyst on a chemical reaction.

Sodium thiosulfate reacts with hydrochloric acid as shown:

Na₂S₂O₃ (aq) + 2HCl (aq) → S (s) + SO₂ (aq) + 2NaCl (aq) + H₂O (l)

The precipitate of sulfur makes the mixture cloudy, so a mark underneath the reaction mixture becomes invisible with time.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Sodium thiosulfate reacts with hydrochloric acid as shown:

Na₂S₂O₃ (aq) + 2HCl (aq) → S (s) + SO₂ (aq) + 2NaCl (aq) + H₂O (l)

The precipitate of sulfur makes the mixture cloudy, so a mark underneath the reaction mixture becomes invisible with time.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Sodium thiosulfate reacts with hydrochloric acid as shown:

Na₂S₂O₃ (aq) + 2HCl (aq) → S (s) + SO₂ (aq) + 2NaCl (aq) + H₂O (l)

The precipitate of sulfur makes the mixture cloudy, so a mark underneath the reaction mixture becomes invisible with time.

Suggest two variables, other than concentration, that should be controlled when comparing relative rates at different temperatures.

Excess magnesium powder was added to a beaker containing hydrochloric acid, HCl (aq).

The mass of the beaker and its contents was recorded and plotted against time (line I).

Which change could give line II?

A. Doubling the mass of powdered Mg

B. Using the same mass of Mg ribbon

C. Increasing the temperature

D. Using the same volume of more concentrated HCl

Excess magnesium powder was added to a beaker containing hydrochloric acid, HCl (aq).

The mass of the beaker and its contents was recorded and plotted against time (line I).

Which change could give line II?

A. Doubling the mass of powdered Mg

B. Using the same mass of Mg ribbon

C. Increasing the temperature

D. Using the same volume of more concentrated HCl

Suggest two variables, besides the time of reaction, which the student should have controlled in the experiment to ensure a fair comparison of the antacids.

Suggest two variables, besides the time of reaction, which the student should have controlled in the experiment to ensure a fair comparison of the antacids.

Suggest two variables, besides the time of reaction, which the student should have controlled in the experiment to ensure a fair comparison of the antacids.

Suggest why point D is so far out of line assuming human error is not the cause.

Suggest why point D is so far out of line assuming human error is not the cause.

Suggest why point D is so far out of line assuming human error is not the cause.

Suggest why point D is so far out of line assuming human error is not the cause.

Suggest why point D is so far out of line assuming human error is not the cause.

Suggest why point D is so far out of line assuming human error is not the cause.

Deduce, giving a reason, which of the two methods would be least affected by the chips not having exactly the same mass when used with the different concentrations of acid.

Deduce, giving a reason, which of the two methods would be least affected by the chips not having exactly the same mass when used with the different concentrations of acid.

Deduce, giving a reason, which of the two methods would be least affected by the chips not having exactly the same mass when used with the different concentrations of acid.

State a factor, that has a significant effect on reaction rate, which could vary between marble chips of exactly the same mass.

State a factor, that has a significant effect on reaction rate, which could vary between marble chips of exactly the same mass.

State a factor, that has a significant effect on reaction rate, which could vary between marble chips of exactly the same mass.

Sketch a Maxwell–Boltzmann distribution curve for a chemical reaction showing the activation energies with and without a catalyst.

Sketch a Maxwell–Boltzmann distribution curve for a chemical reaction showing the activation energies with and without a catalyst.

Sketch a Maxwell–Boltzmann distribution curve for a chemical reaction showing the activation energies with and without a catalyst.

Explain why aspirin is not stored in a hot, humid location.

Explain why aspirin is not stored in a hot, humid location.

Explain why aspirin is not stored in a hot, humid location.

Samples of sodium carbonate powder were reacted with separate samples of excess hydrochloric acid.

Na₂CO₃ (s) + 2HCl (aq) → CO₂ (g) + 2NaCl (aq) + H₂O (l)

Reaction I: 1.0 g Na₂CO₃ (s) added to 0.50 mol dm⁻³ HCl (aq)

Reaction II: 1.0 g Na₂CO₃ (s) added to 2.0 mol dm⁻³ HCl (aq)

What is the same for reactions I and II?

A.   Initial rate of reaction

B.   Total mass of CO₂ produced

C.   Total reaction time

D.   Average rate of production of CO₂

Samples of sodium carbonate powder were reacted with separate samples of excess hydrochloric acid.

Na₂CO₃ (s) + 2HCl (aq) → CO₂ (g) + 2NaCl (aq) + H₂O (l)

Reaction I: 1.0 g Na₂CO₃ (s) added to 0.50 mol dm⁻³ HCl (aq)

Reaction II: 1.0 g Na₂CO₃ (s) added to 2.0 mol dm⁻³ HCl (aq)

What is the same for reactions I and II?

A.   Initial rate of reaction

B.   Total mass of CO₂ produced

C.   Total reaction time

D.   Average rate of production of CO₂

Outline how the initial rate of reaction can be determined from the graph in part (c)(i).

Outline how the initial rate of reaction can be determined from the graph in part (c)(i).

Outline how the initial rate of reaction can be determined from the graph in part (c)(i).

Outline how the initial rate of reaction can be determined from the graph in part (c)(i).

Outline how the initial rate of reaction can be determined from the graph in part (c)(i).

Outline how the initial rate of reaction can be determined from the graph in part (c)(i).

Apart from a greater frequency of collisions, explain, by annotating your graphs in (b)(iii), why an increased temperature causes the rate of reaction to increase.

Apart from a greater frequency of collisions, explain, by annotating your graphs in (b)(iii), why an increased temperature causes the rate of reaction to increase.

Apart from a greater frequency of collisions, explain, by annotating your graphs in (b)(iii), why an increased temperature causes the rate of reaction to increase.

Outline, in terms of collision theory, how a decrease in pressure would affect the rate of reaction.

Outline, in terms of collision theory, how a decrease in pressure would affect the rate of reaction.

Outline, in terms of collision theory, how a decrease in pressure would affect the rate of reaction.

The experiment is repeated using the same amount of dinitrogen monoxide in the same apparatus, but at a lower temperature.

Sketch, on the axes in question 2, the graph that you would expect.

The experiment is repeated using the same amount of dinitrogen monoxide in the same apparatus, but at a lower temperature.

Sketch, on the axes in question 2, the graph that you would expect.

The experiment is repeated using the same amount of dinitrogen monoxide in the same apparatus, but at a lower temperature.

Sketch, on the axes in question 2, the graph that you would expect.

Identify the experiment with the highest rate of lead dissolving.

Identify the experiment with the highest rate of lead dissolving.

Identify the experiment with the highest rate of lead dissolving.

Outline, with a reason, another property that could be monitored to measure the rate of this reaction.

Outline, with a reason, another property that could be monitored to measure the rate of this reaction.

Outline, with a reason, another property that could be monitored to measure the rate of this reaction.

The dotted line represents the formation of oxygen, O₂ (g), from the uncatalysed complete decomposition of hydrogen peroxide, H₂O₂ (aq).

Which curve represents a catalysed reaction under the same conditions?

The dotted line represents the formation of oxygen, O₂ (g), from the uncatalysed complete decomposition of hydrogen peroxide, H₂O₂ (aq).

Which curve represents a catalysed reaction under the same conditions?

Several reactions of calcium carbonate with dilute hydrochloric acid are carried out at the same temperature.

CaCO₃ (s) + 2HCl (aq) → CaCl₂ (aq) + H₂O (l) + CO₂ (g)

Which reaction has the greatest rate?

Several reactions of calcium carbonate with dilute hydrochloric acid are carried out at the same temperature.

CaCO₃ (s) + 2HCl (aq) → CaCl₂ (aq) + H₂O (l) + CO₂ (g)

Which reaction has the greatest rate?

Additional experiments were carried out at an elevated temperature. On the axes below, sketch Maxwell–Boltzmann energy distribution curves at two temperatures T₁ and T₂, where T₂ > T₁.

Additional experiments were carried out at an elevated temperature. On the axes below, sketch Maxwell–Boltzmann energy distribution curves at two temperatures T₁ and T₂, where T₂ > T₁.

Additional experiments were carried out at an elevated temperature. On the axes below, sketch Maxwell–Boltzmann energy distribution curves at two temperatures T₁ and T₂, where T₂ > T₁.

Apart from a greater frequency of collisions, explain, by annotating your graphs in (b)(ii), why an increased temperature causes the rate of reaction to increase.

Apart from a greater frequency of collisions, explain, by annotating your graphs in (b)(ii), why an increased temperature causes the rate of reaction to increase.

Apart from a greater frequency of collisions, explain, by annotating your graphs in (b)(ii), why an increased temperature causes the rate of reaction to increase.

Outline, in terms of collision theory, how a decrease in pressure would affect the rate of reaction.

Outline, in terms of collision theory, how a decrease in pressure would affect the rate of reaction.

Outline, in terms of collision theory, how a decrease in pressure would affect the rate of reaction.

The experiment is repeated using the same amount of dinitrogen monoxide in the same apparatus, but at a lower temperature.

Sketch, on the axes in question 2, the graph that you would expect.

The experiment is repeated using the same amount of dinitrogen monoxide in the same apparatus, but at a lower temperature.

Sketch, on the axes in question 2, the graph that you would expect.

The experiment is repeated using the same amount of dinitrogen monoxide in the same apparatus, but at a lower temperature.

Sketch, on the axes in question 2, the graph that you would expect.

The graph below shows the Maxwell–Boltzmann distribution of molecular energies at a particular temperature.

The rate at which dinitrogen monoxide decomposes is significantly increased by a metal oxide catalyst.

Annotate and use the graph to outline why a catalyst has this effect.

The graph below shows the Maxwell–Boltzmann distribution of molecular energies at a particular temperature.

The rate at which dinitrogen monoxide decomposes is significantly increased by a metal oxide catalyst.

Annotate and use the graph to outline why a catalyst has this effect.

The graph below shows the Maxwell–Boltzmann distribution of molecular energies at a particular temperature.

The rate at which dinitrogen monoxide decomposes is significantly increased by a metal oxide catalyst.

Annotate and use the graph to outline why a catalyst has this effect.

Identify the experiment with the highest rate of lead dissolving.

Identify the experiment with the highest rate of lead dissolving.

Identify the experiment with the highest rate of lead dissolving.

Determine from the graph the rate of reaction at 20 s, in cm³ s⁻¹, showing your working.

Determine from the graph the rate of reaction at 20 s, in cm³ s⁻¹, showing your working.

Determine from the graph the rate of reaction at 20 s, in cm³ s⁻¹, showing your working.

Outline, with a reason, another property that could be monitored to measure the rate of this reaction.

Outline, with a reason, another property that could be monitored to measure the rate of this reaction.

Outline, with a reason, another property that could be monitored to measure the rate of this reaction.

The dotted line represents the formation of oxygen, O₂(g), from the uncatalysed complete decomposition of hydrogen peroxide, H₂O₂ (aq).

Which curve represents a catalysed reaction under the same conditions?

The dotted line represents the formation of oxygen, O₂(g), from the uncatalysed complete decomposition of hydrogen peroxide, H₂O₂ (aq).

Which curve represents a catalysed reaction under the same conditions?

Several reactions of calcium carbonate with dilute hydrochloric acid are carried out at the same temperature.

CaCO₃ (s) + 2HCl (aq) → CaCl₂ (aq) + H₂O (l) + CO₂ (g)

Which reaction has the greatest rate?

Several reactions of calcium carbonate with dilute hydrochloric acid are carried out at the same temperature.

CaCO₃ (s) + 2HCl (aq) → CaCl₂ (aq) + H₂O (l) + CO₂ (g)

Which reaction has the greatest rate?

Determine the initial rate of reaction of limestone with nitric acid from the graph.

Show your working on the graph and include the units of the initial rate.

Determine the initial rate of reaction of limestone with nitric acid from the graph.

Show your working on the graph and include the units of the initial rate.

Determine the initial rate of reaction of limestone with nitric acid from the graph.

Show your working on the graph and include the units of the initial rate.

Explain why the rate of reaction of limestone with nitric acid decreases and reaches zero over the period of five days.

Explain why the rate of reaction of limestone with nitric acid decreases and reaches zero over the period of five days.

Explain why the rate of reaction of limestone with nitric acid decreases and reaches zero over the period of five days.

Which apparatus can be used to monitor the rate of this reaction?

${\mathrm{CH}}_3{\mathrm{COCH}}_3 \left(\mathrm{aq}\right)+{\mathrm{I}}_2 \left(\mathrm{aq}\right)\to {\mathrm{CH}}_3{\mathrm{COCH}}_2\mathrm{I} \left(\mathrm{aq}\right)+{\mathrm{H}}^{+} \left(\mathrm{aq}\right)+{\mathrm{I}}^{-} \left(\mathrm{aq}\right)$

1. A pH meter
2. A gas syringe
3. A colorimeter
   

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which apparatus can be used to monitor the rate of this reaction?

${\mathrm{CH}}_3{\mathrm{COCH}}_3 \left(\mathrm{aq}\right)+{\mathrm{I}}_2 \left(\mathrm{aq}\right)\to {\mathrm{CH}}_3{\mathrm{COCH}}_2\mathrm{I} \left(\mathrm{aq}\right)+{\mathrm{H}}^{+} \left(\mathrm{aq}\right)+{\mathrm{I}}^{-} \left(\mathrm{aq}\right)$

1. A pH meter
2. A gas syringe
3. A colorimeter
   

A.  I and II only

B.  I and III only

C.  II and III only

D.  I, II and III

Which arrow shows the activation energy of the uncatalysed forward reaction for this equilibrium?

$2{\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$     $∆H=-196 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Which arrow shows the activation energy of the uncatalysed forward reaction for this equilibrium?

$2{\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$     $∆H=-196 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Which change does not increase the rate of this reaction?

${\mathrm{CuCO}}_3 \left(\mathrm{s}\right)+{\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)\to {\mathrm{CuSO}}_4 \left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)+{\mathrm{CO}}_2 \left(\mathrm{g}\right)$

A.  Increasing the particle size of the ${\mathrm{CuCO}}_3$

B.  Increasing the temperature

C.  Increasing the concentration of ${\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)$

D.  Stirring the reaction mixture

Which change does not increase the rate of this reaction?

${\mathrm{CuCO}}_3 \left(\mathrm{s}\right)+{\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)\to {\mathrm{CuSO}}_4 \left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)+{\mathrm{CO}}_2 \left(\mathrm{g}\right)$

A.  Increasing the particle size of the ${\mathrm{CuCO}}_3$

B.  Increasing the temperature

C.  Increasing the concentration of ${\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)$

D.  Stirring the reaction mixture

Explain why an increase in temperature increases the rate of reaction.

Explain why an increase in temperature increases the rate of reaction.

Explain why an increase in temperature increases the rate of reaction.

The diagram shows the Maxwell-Boltzmann curve for the uncatalyzed reaction.

Draw a distribution curve at a lower temperature (T₂) and show on the diagram how the addition of a catalyst enables the reaction to take place more rapidly than at T₁.

The diagram shows the Maxwell-Boltzmann curve for the uncatalyzed reaction.

Draw a distribution curve at a lower temperature (T₂) and show on the diagram how the addition of a catalyst enables the reaction to take place more rapidly than at T₁.

The diagram shows the Maxwell-Boltzmann curve for the uncatalyzed reaction.

Draw a distribution curve at a lower temperature (T₂) and show on the diagram how the addition of a catalyst enables the reaction to take place more rapidly than at T₁.

Deduce the relationship between the concentration of N₂O₅ and the rate of reaction.

Deduce the relationship between the concentration of N₂O₅ and the rate of reaction.

Deduce the relationship between the concentration of N₂O₅ and the rate of reaction.

Sketch labelled Maxwell–Boltzmann energy distribution curves at the original temperature (T₁) and the new lower temperature (T₂).

Sketch labelled Maxwell–Boltzmann energy distribution curves at the original temperature (T₁) and the new lower temperature (T₂).

Sketch labelled Maxwell–Boltzmann energy distribution curves at the original temperature (T₁) and the new lower temperature (T₂).

Outline, giving a reason, the effect of a catalyst on a reaction.

Outline, giving a reason, the effect of a catalyst on a reaction.

Outline, giving a reason, the effect of a catalyst on a reaction.

What is the enthalpy change for the following reaction?

CH₄ (g) + H₂O (g) → CO (g) + 3H₂ (g)

A.  −74 − 242 + 111

B.  +74 + 242 − 111

C.  −74 − 484 − 222

D.  +74 + 484 − 222

What is the enthalpy change for the following reaction?

CH₄ (g) + H₂O (g) → CO (g) + 3H₂ (g)

A.  −74 − 242 + 111

B.  +74 + 242 − 111

C.  −74 − 484 − 222

D.  +74 + 484 − 222

What are the numbers of neutrons and electrons in ${}_{16}{}^{32}\mathrm{S}_{2-}$?

What are the numbers of neutrons and electrons in ${}_{16}{}^{32}\mathrm{S}_{2-}$?