DP Chemistry (first assessment 2025)

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Reactivity 2. How much, how fast and how far? » Reactivity 2.3—How far? The extent of chemical change » Reactivity 2.3.7—The equilibrium constant and Gibbs energy change, ΔG, can both be used to measure the position of an equilibrium reaction.

Reactivity 2.3.7—The equilibrium constant and Gibbs energy change, ΔG, can both be used to measure the position of an equilibrium reaction.

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Directly related questions

19M.1A.HL.TZ1.23: Which is correct for a reaction with a positive change in Gibbs free energy, ΔGθ? A. The...
19M.1A.HL.TZ1.23: Which is correct for a reaction with a positive change in Gibbs free energy, ΔGθ? A. The...
19M.1A.HL.TZ1.23: Which is correct for a reaction with a positive change in Gibbs free energy, ΔGθ? A. The...
19M.1A.HL.TZ1.23: Which is correct for a reaction with a positive change in Gibbs free energy, ΔGθ? A. The...
19M.2.HL.TZ2.6b:
Phenylethene is manufactured from benzene and ethene in a two-stage process. The overall reaction can be represented as follows with ΔG^θ = +10.0 kJ mol⁻¹ at 298 K.

Calculate the equilibrium constant for the overall conversion at 298 K, using section 1 of the data booklet.
19M.2.HL.TZ2.6b:
Phenylethene is manufactured from benzene and ethene in a two-stage process. The overall reaction can be represented as follows with ΔG^θ = +10.0 kJ mol⁻¹ at 298 K.

Calculate the equilibrium constant for the overall conversion at 298 K, using section 1 of the data booklet.
19M.2.HL.TZ2.b:
Phenylethene is manufactured from benzene and ethene in a two-stage process. The overall reaction can be represented as follows with ΔG^θ = +10.0 kJ mol⁻¹ at 298 K.

Calculate the equilibrium constant for the overall conversion at 298 K, using section 1 of the data booklet.
19M.2.HL.TZ2.6b:
Phenylethene is manufactured from benzene and ethene in a two-stage process. The overall reaction can be represented as follows with ΔG^θ = +10.0 kJ mol⁻¹ at 298 K.

Calculate the equilibrium constant for the overall conversion at 298 K, using section 1 of the data booklet.
19M.2.HL.TZ2.6b:
Phenylethene is manufactured from benzene and ethene in a two-stage process. The overall reaction can be represented as follows with ΔG^θ = +10.0 kJ mol⁻¹ at 298 K.

Calculate the equilibrium constant for the overall conversion at 298 K, using section 1 of the data booklet.
19M.2.HL.TZ2.b:
Phenylethene is manufactured from benzene and ethene in a two-stage process. The overall reaction can be represented as follows with ΔG^θ = +10.0 kJ mol⁻¹ at 298 K.

Calculate the equilibrium constant for the overall conversion at 298 K, using section 1 of the data booklet.
19N.2.HL.TZ0.4a(iv):
Calculate the standard Gibbs free energy change, $\Delta {G^\theta }$ , in kJ mol⁻¹, for the first dissociation of citric acid at 298 K, using section 1 of the data booklet.
19N.2.HL.TZ0.4a(iv):
Calculate the standard Gibbs free energy change, $\Delta {G^\theta }$ , in kJ mol⁻¹, for the first dissociation of citric acid at 298 K, using section 1 of the data booklet.
19N.2.HL.TZ0.a(iv):
Calculate the standard Gibbs free energy change, $\Delta {G^\theta }$ , in kJ mol⁻¹, for the first dissociation of citric acid at 298 K, using section 1 of the data booklet.
19N.2.HL.TZ0.4a(iv):
Calculate the standard Gibbs free energy change, $\Delta {G^\theta }$ , in kJ mol⁻¹, for the first dissociation of citric acid at 298 K, using section 1 of the data booklet.
19N.2.HL.TZ0.4a(iv):
Calculate the standard Gibbs free energy change, $\Delta {G^\theta }$ , in kJ mol⁻¹, for the first dissociation of citric acid at 298 K, using section 1 of the data booklet.
19N.2.HL.TZ0.a(iv):
Calculate the standard Gibbs free energy change, $\Delta {G^\theta }$ , in kJ mol⁻¹, for the first dissociation of citric acid at 298 K, using section 1 of the data booklet.
20N.1A.HL.TZ0.23: Which statement is correct for a spontaneous reaction?
20N.1A.HL.TZ0.23: Which statement is correct for a spontaneous reaction?
20N.1A.HL.TZ0.23: Which statement is correct for a spontaneous reaction?
20N.1A.HL.TZ0.23: Which statement is correct for a spontaneous reaction?
22M.2.HL.TZ1.3c(i): State, giving a reason, whether the reaction is spontaneous or not at 298 K.
22M.2.HL.TZ1.3c(i): State, giving a reason, whether the reaction is spontaneous or not at 298 K.
22M.2.HL.TZ1.c(i): State, giving a reason, whether the reaction is spontaneous or not at 298 K.
22M.2.HL.TZ1.3c(i): State, giving a reason, whether the reaction is spontaneous or not at 298 K.
22M.2.HL.TZ1.3c(i): State, giving a reason, whether the reaction is spontaneous or not at 298 K.
22M.2.HL.TZ1.c(i): State, giving a reason, whether the reaction is spontaneous or not at 298 K.
22M.2.HL.TZ1.3c(ii):
Calculate the value of the equilibrium constant, K, at 298 K. Use sections 1 and 2 of the data booklet.
22M.2.HL.TZ1.3c(ii):
Calculate the value of the equilibrium constant, K, at 298 K. Use sections 1 and 2 of the data booklet.
22M.2.HL.TZ1.c(ii):
Calculate the value of the equilibrium constant, K, at 298 K. Use sections 1 and 2 of the data booklet.
22M.2.HL.TZ1.3c(ii):
Calculate the value of the equilibrium constant, K, at 298 K. Use sections 1 and 2 of the data booklet.
22M.2.HL.TZ1.3c(ii):
Calculate the value of the equilibrium constant, K, at 298 K. Use sections 1 and 2 of the data booklet.
22M.2.HL.TZ1.c(ii):
Calculate the value of the equilibrium constant, K, at 298 K. Use sections 1 and 2 of the data booklet.

Sub sections and their related questions

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