1. Consider the following equilibrium: H2O(g) + CO(g) â H2(g) + CO2(g)
A closed container is initially filled with H2O and CO. As the reaction proceeds towards equilibrium the
A. [CO] and [CO2] both increase
B. [ CO] and [CO2] both decrease
C. [CO] increases and [CO2] decreases
D. [CO] decreases and [CO2] increases
2. Consider the following equilibrium: 2SO3(g) â 2SO2(g) + O2(g)
At equilibrium, the rate of decomposition of SO3
A. Equals the rate of formation of O2
B. Equals the rate of formation of SO3
C. Is less than the rate of formation of O2
D. Is less than the rate of formation of SO3
3. Which of the following is true for all equilibrium systems?
A. The mass of reactants is equal to the mass of products
B. Addition of a catalyst changes the equilibrium concentrations
C. The concentration of reactants is equal to the concentration of products
D. The rate of the forward reaction is equal to the rate of the reverse reaction
1. Consider the following equilibrium: H2O(g) + CO(g) â H2(g) + CO2(g)
A closed container is initially filled with H2O and CO. As the reaction proceeds towards equilibrium the
A. [CO] and [CO2] both increase
B. [ CO] and [CO2] both decrease
C. [CO] increases and [CO2] decreases
D. [CO] decreases and [CO2] increases
2. Consider the following equilibrium: 2SO3(g) â 2SO2(g) + O2(g)
At equilibrium, the rate of decomposition of SO3
A. Equals the rate of formation of O2
B. Equals the rate of formation of SO3
C. Is less than the rate of formation of O2
D. Is less than the rate of formation of SO3
3. Which of the following is true for all equilibrium systems?
A. The mass of reactants is equal to the mass of products
B. Addition of a catalyst changes the equilibrium concentrations
C. The concentration of reactants is equal to the concentration of products
D. The rate of the forward reaction is equal to the rate of the reverse reaction