Given the equilibrium reaction:
ZnCO3(s) ZnO(s) + CO2(g)
Which one of the following statements is true?
a. Equal concentrations of ZnO(s) and CO2(g) would result from the decomposition of a given amount of ZnCO3(s).
b. The same equilibrium condition would result if we started with only pure ZnCO3(s) in a closed container as if we started with only pure ZnO(s) in a closed container.
c. Introducing 1.0 atm pressure of N2(g) into the system at equilibrium in a closed container would result in more ZnCO3(s) being formed.
d. Decreasing the volume of the closed system initially at equilibrium, at constant temperature, would result in more ZnCO3(s) being formed.
e. At equilibrium conditions, the forward and reverse reactions have stopped.
Answer: d. Decreasing the volume of the closed system initially at equilibrium, at constant temperature, would result in more ZnCO3(s) being formed.