Structure 1.5.4—The relationship between the pressure, volume, temperature and amount of an ideal gas is shown in the ideal gas equation PV = nRT and the combined gas law P1V1T1= P2V2T2. Solve problems relating to the ideal gas equation.

Which volume of ethane gas, in ${\mathrm{cm}}^3$, will produce $40 {\mathrm{cm}}^3$ of carbon dioxide gas when mixed with $140 {\mathrm{cm}}^3$ of oxygen gas, assuming the reaction goes to completion?

$2{\mathrm{C}}_2{\mathrm{H}}_6 \left(\mathrm{g}\right)+7{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2 \left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$

A.  $10$

B.  $20$

C.  $40$

D.  $80$

Which volume of ethane gas, in ${\mathrm{cm}}^3$, will produce $40 {\mathrm{cm}}^3$ of carbon dioxide gas when mixed with $140 {\mathrm{cm}}^3$ of oxygen gas, assuming the reaction goes to completion?

$2{\mathrm{C}}_2{\mathrm{H}}_6 \left(\mathrm{g}\right)+7{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2 \left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$

A.  $10$

B.  $20$

C.  $40$

D.  $80$

Which volume of ethane gas, in ${\mathrm{cm}}^3$, will produce $40 {\mathrm{cm}}^3$ of carbon dioxide gas when mixed with $140 {\mathrm{cm}}^3$ of oxygen gas, assuming the reaction goes to completion?

$2{\mathrm{C}}_2{\mathrm{H}}_6 \left(\mathrm{g}\right)+7{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2 \left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$

A.  $10$

B.  $20$

C.  $40$

D.  $80$

Which volume of ethane gas, in ${\mathrm{cm}}^3$, will produce $40 {\mathrm{cm}}^3$ of carbon dioxide gas when mixed with $140 {\mathrm{cm}}^3$ of oxygen gas, assuming the reaction goes to completion?

$2{\mathrm{C}}_2{\mathrm{H}}_6 \left(\mathrm{g}\right)+7{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2 \left(\mathrm{g}\right)+6{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)$

A.  $10$

B.  $20$

C.  $40$

D.  $80$

The vapour pressure of pure ethanal at $20°\mathrm{C}$ is $101 \mathrm{kPa}$.

Calculate the vapour pressure of ethanal above the liquid mixture at $20°\mathrm{C}$.

The vapour pressure of pure ethanal at $20°\mathrm{C}$ is $101 \mathrm{kPa}$.

Calculate the vapour pressure of ethanal above the liquid mixture at $20°\mathrm{C}$.

The vapour pressure of pure ethanal at $20°\mathrm{C}$ is $101 \mathrm{kPa}$.

Calculate the vapour pressure of ethanal above the liquid mixture at $20°\mathrm{C}$.

The vapour pressure of pure ethanal at $20°\mathrm{C}$ is $101 \mathrm{kPa}$.

Calculate the vapour pressure of ethanal above the liquid mixture at $20°\mathrm{C}$.

What volume of oxygen, in dm³ at STP, is needed when 5.8 g of butane undergoes complete combustion?

$2{\mathrm{C}}_4{\mathrm{H}}_{10} \left(\mathrm{g}\right)+13{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 8{\mathrm{CO}}_2 \left(\mathrm{g}\right)+10{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

A.  $2\times \frac{5.8}{12.01\times 4+1.01\times 10}\times 13\times 22.7$

B.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times 22.7$

C.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{2}{13}\times 22.7$

D.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times \frac{22.7}{1000}$

What volume of oxygen, in dm³ at STP, is needed when 5.8 g of butane undergoes complete combustion?

$2{\mathrm{C}}_4{\mathrm{H}}_{10} \left(\mathrm{g}\right)+13{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 8{\mathrm{CO}}_2 \left(\mathrm{g}\right)+10{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

A.  $2\times \frac{5.8}{12.01\times 4+1.01\times 10}\times 13\times 22.7$

B.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times 22.7$

C.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{2}{13}\times 22.7$

D.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times \frac{22.7}{1000}$

What volume of oxygen, in dm³ at STP, is needed when 5.8 g of butane undergoes complete combustion?

$2{\mathrm{C}}_4{\mathrm{H}}_{10} \left(\mathrm{g}\right)+13{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 8{\mathrm{CO}}_2 \left(\mathrm{g}\right)+10{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

A.  $2\times \frac{5.8}{12.01\times 4+1.01\times 10}\times 13\times 22.7$

B.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times 22.7$

C.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{2}{13}\times 22.7$

D.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times \frac{22.7}{1000}$

What volume of oxygen, in dm³ at STP, is needed when 5.8 g of butane undergoes complete combustion?

$2{\mathrm{C}}_4{\mathrm{H}}_{10} \left(\mathrm{g}\right)+13{\mathrm{O}}_2 \left(\mathrm{g}\right)\to 8{\mathrm{CO}}_2 \left(\mathrm{g}\right)+10{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

A.  $2\times \frac{5.8}{12.01\times 4+1.01\times 10}\times 13\times 22.7$

B.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times 22.7$

C.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{2}{13}\times 22.7$

D.  $\frac{5.8}{12.01\times 4+1.01\times 10}\times \frac{13}{2}\times \frac{22.7}{1000}$

Calcium carbonate is heated to produce calcium oxide, CaO.

CaCO₃(s) → CaO (s) + CO₂(g)

Calculate the volume of carbon dioxide produced at STP when 555 g of calcium carbonate decomposes. Use sections 2 and 6 of the data booklet.

Calcium carbonate is heated to produce calcium oxide, CaO.

CaCO₃(s) → CaO (s) + CO₂(g)

Calculate the volume of carbon dioxide produced at STP when 555 g of calcium carbonate decomposes. Use sections 2 and 6 of the data booklet.

Calcium carbonate is heated to produce calcium oxide, CaO.

CaCO₃(s) → CaO (s) + CO₂(g)

Calculate the volume of carbon dioxide produced at STP when 555 g of calcium carbonate decomposes. Use sections 2 and 6 of the data booklet.

Calcium carbonate is heated to produce calcium oxide, CaO.

CaCO₃(s) → CaO (s) + CO₂(g)

Calculate the volume of carbon dioxide produced at STP when 555 g of calcium carbonate decomposes. Use sections 2 and 6 of the data booklet.

Calcium carbonate is heated to produce calcium oxide, CaO.

CaCO₃(s) → CaO (s) + CO₂(g)

Calculate the volume of carbon dioxide produced at STP when 555 g of calcium carbonate decomposes. Use sections 2 and 6 of the data booklet.

Calcium carbonate is heated to produce calcium oxide, CaO.

CaCO₃(s) → CaO (s) + CO₂(g)

Calculate the volume of carbon dioxide produced at STP when 555 g of calcium carbonate decomposes. Use sections 2 and 6 of the data booklet.

Determine the mass, in g, of CaCO₃(s) produced by reacting 2.41 dm³ of 2.33 × 10⁻² mol dm⁻³ of Ca(OH)₂ (aq) with 0.750 dm³ of CO₂ (g) at STP.

Determine the mass, in g, of CaCO₃(s) produced by reacting 2.41 dm³ of 2.33 × 10⁻² mol dm⁻³ of Ca(OH)₂ (aq) with 0.750 dm³ of CO₂ (g) at STP.

Determine the mass, in g, of CaCO₃(s) produced by reacting 2.41 dm³ of 2.33 × 10⁻² mol dm⁻³ of Ca(OH)₂ (aq) with 0.750 dm³ of CO₂ (g) at STP.

Determine the mass, in g, of CaCO₃(s) produced by reacting 2.41 dm³ of 2.33 × 10⁻² mol dm⁻³ of Ca(OH)₂ (aq) with 0.750 dm³ of CO₂ (g) at STP.

Determine the mass, in g, of CaCO₃(s) produced by reacting 2.41 dm³ of 2.33 × 10⁻² mol dm⁻³ of Ca(OH)₂ (aq) with 0.750 dm³ of CO₂ (g) at STP.

Determine the mass, in g, of CaCO₃(s) produced by reacting 2.41 dm³ of 2.33 × 10⁻² mol dm⁻³ of Ca(OH)₂ (aq) with 0.750 dm³ of CO₂ (g) at STP.

2.85 g of CaCO₃ was collected in the experiment in d(i). Calculate the percentage yield of CaCO₃.

(If you did not obtain an answer to d(i), use 4.00 g, but this is not the correct value.)

2.85 g of CaCO₃ was collected in the experiment in d(i). Calculate the percentage yield of CaCO₃.

(If you did not obtain an answer to d(i), use 4.00 g, but this is not the correct value.)

2.85 g of CaCO₃ was collected in the experiment in d(i). Calculate the percentage yield of CaCO₃.

(If you did not obtain an answer to d(i), use 4.00 g, but this is not the correct value.)

2.85 g of CaCO₃ was collected in the experiment in d(i). Calculate the percentage yield of CaCO₃.

(If you did not obtain an answer to d(i), use 4.00 g, but this is not the correct value.)

2.85 g of CaCO₃ was collected in the experiment in d(i). Calculate the percentage yield of CaCO₃.

(If you did not obtain an answer to d(i), use 4.00 g, but this is not the correct value.)

2.85 g of CaCO₃ was collected in the experiment in d(i). Calculate the percentage yield of CaCO₃.

(If you did not obtain an answer to d(i), use 4.00 g, but this is not the correct value.)