Ammonia is prepared industrially by the following reaction:
N2(g) + 3H2(g) ⇌ 2NH3(g)
ΔH° = -92.2 kJ and Kc (at 25°C) = 4.0 x 10^8
When the temperature is increased to 500°C, which of the following is true?
a. Kc value for the reaction is larger at 500°C than at 25°C.
b. The reaction of N2 with H2 to form NH3 is endothermic.
c. Product formation at equilibrium is not favored as the temperature increases.
Given sufficient activation energy, which statements about a dynamic equilibrium are correct?
a. At equilibrium, the forward and reverse reactions are occurring at the same rate.
b. The equilibrium constant is altered when the pressure of the system changes.
c. An equilibrium constant that is much smaller than 1 suggests that the equilibrium mixture favors the reactants.
Which of the following equilibria will shift to the left if the pressure of the system is decreased?
a. NH4NO3(s) ⇌ N2O(g) + 2H2O(g)
b. 4NH3(g) + 5O2(g) ⇌ 4NO(g) + 6H2O(g)
c. Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g)
d. 2SO2(g) + O2(g) ⇌ 2SO3(g)
e. 2HF(g) ⇌ H2(g) + F2(g)
When carbon dioxide is mixed with hot carbon, the following equilibrium is established:
C(s) + CO2(g) ⇌ 2CO(g) Kc = 13.8
If the equilibrium concentration of carbon dioxide is found to be 0.0248 M, what is the equilibrium concentration of carbon monoxide?
a. 0.171 M
b. 0.342 M
c. 0.0496 M
d. 0.0423 M
e. 0.585 M