Reactivity 2.3.3—The magnitude of the equilibrium constant indicates the extent of a reaction at equilibrium and is temperature dependent. Determine the relationships between K values for reactions that are the reverse of each other at the same temperature.
Description
[N/A]Directly related questions
- 21N.1A.SL.TZ0.27: What is correct for pure hot water?
- 21N.1A.SL.TZ0.27: What is correct for pure hot water?
- 21N.1A.SL.TZ0.27: What is correct for pure hot water?
- 21N.1A.SL.TZ0.27: What is correct for pure hot water?
-
21N.1A.SL.TZ0.19:
The equilibrium 2H2 (g) + N2 (g) N2H4 (g) has an equilibrium constant, K, at 150 °C.
What is the equilibrium constant at 150 °C, for the reverse reaction?
N2H4 (g) 2H2 (g) + N2 (g)
A. KB. K−1
C. −K
D. 2K
-
21N.1A.SL.TZ0.19:
The equilibrium 2H2 (g) + N2 (g) N2H4 (g) has an equilibrium constant, K, at 150 °C.
What is the equilibrium constant at 150 °C, for the reverse reaction?
N2H4 (g) 2H2 (g) + N2 (g)
A. KB. K−1
C. −K
D. 2K
-
21N.1A.SL.TZ0.19:
The equilibrium 2H2 (g) + N2 (g) N2H4 (g) has an equilibrium constant, K, at 150 °C.
What is the equilibrium constant at 150 °C, for the reverse reaction?
N2H4 (g) 2H2 (g) + N2 (g)
A. KB. K−1
C. −K
D. 2K
-
21N.1A.SL.TZ0.19:
The equilibrium 2H2 (g) + N2 (g) N2H4 (g) has an equilibrium constant, K, at 150 °C.
What is the equilibrium constant at 150 °C, for the reverse reaction?
N2H4 (g) 2H2 (g) + N2 (g)
A. KB. K−1
C. −K
D. 2K
-
22M.1A.SL.TZ2.20:
What is the strongest acid in the equation below?
H3AsO4 + H2O H2AsO4− + H3O+ Kc = 4.5 × 10−4
A. H3AsO4
B. H2O
C. H2AsO4−
D. H3O+
-
22M.1A.SL.TZ2.20:
What is the strongest acid in the equation below?
H3AsO4 + H2O H2AsO4− + H3O+ Kc = 4.5 × 10−4
A. H3AsO4
B. H2O
C. H2AsO4−
D. H3O+
-
22M.1A.SL.TZ2.20:
What is the strongest acid in the equation below?
H3AsO4 + H2O H2AsO4− + H3O+ Kc = 4.5 × 10−4
A. H3AsO4
B. H2O
C. H2AsO4−
D. H3O+
-
22M.1A.SL.TZ2.20:
What is the strongest acid in the equation below?
H3AsO4 + H2O H2AsO4− + H3O+ Kc = 4.5 × 10−4
A. H3AsO4
B. H2O
C. H2AsO4−
D. H3O+
-
22M.2.SL.TZ1.3b(i):
Determine the enthalpy change, ΔH, for the Haber–Bosch process, in kJ. Use Section 11 of the data booklet.
-
22M.2.SL.TZ1.3b(i):
Determine the enthalpy change, ΔH, for the Haber–Bosch process, in kJ. Use Section 11 of the data booklet.
-
22M.2.SL.TZ1.b(i):
Determine the enthalpy change, ΔH, for the Haber–Bosch process, in kJ. Use Section 11 of the data booklet.
-
22M.2.SL.TZ1.3b(i):
Determine the enthalpy change, ΔH, for the Haber–Bosch process, in kJ. Use Section 11 of the data booklet.
-
22M.2.SL.TZ1.3b(i):
Determine the enthalpy change, ΔH, for the Haber–Bosch process, in kJ. Use Section 11 of the data booklet.
-
22M.2.SL.TZ1.b(i):
Determine the enthalpy change, ΔH, for the Haber–Bosch process, in kJ. Use Section 11 of the data booklet.
-
22M.2.SL.TZ1.3b(iii):
Demonstrate that your answer to (b)(i) is consistent with the effect of an increase in temperature on the percentage yield, as shown in the graph.
-
22M.2.SL.TZ1.3b(iii):
Demonstrate that your answer to (b)(i) is consistent with the effect of an increase in temperature on the percentage yield, as shown in the graph.
-
22M.2.SL.TZ1.b(iii):
Demonstrate that your answer to (b)(i) is consistent with the effect of an increase in temperature on the percentage yield, as shown in the graph.
-
22M.2.SL.TZ1.3b(iii):
Demonstrate that your answer to (b)(i) is consistent with the effect of an increase in temperature on the percentage yield, as shown in the graph.
-
22M.2.SL.TZ1.3b(iii):
Demonstrate that your answer to (b)(i) is consistent with the effect of an increase in temperature on the percentage yield, as shown in the graph.
-
22M.2.SL.TZ1.b(iii):
Demonstrate that your answer to (b)(i) is consistent with the effect of an increase in temperature on the percentage yield, as shown in the graph.