The units of the rate depend on the order of the reaction.

The half-life of a second-order reaction does not depend on the initial concentration of reactant

The greater the energy of activation, Ea, the faster the reaction will be

The rate of a reaction is determined by the rate of the fastest step in the mechanism.

When a reaction system reaches equilibrium, the concentrations of reactants and products no longer change

If Q>K, more products need to be formed as the reaction proceeds to equilibrium

Consider the reaction:

2NH₃(g) --> N₂(g) + 3H₂(g)

If the rate for the appearance of H₂ is 0.030 mol/Ls, then what is the rate of decrease of NH₃?

Which of the following sets of units could be appropriate for a zero-order rate constant?

A reaction is second-order with respect tot he reactant R. Which of the following plots will produce a straight line?

The rate constant for the reaction 3A --> 4B is 6.00 x 10^-3 L/mol min. How long will it take the concentration of A to drop from 0.75 M to 0.25 M?

Which of the following affects the activation energy of a reaction?

The equilibrium constant, Kc, for the decomposition of COBr₂ is 0.190.

COBr₂ ↔ CO + Br₂

What is the Kc for the following reaction?

2CO + 2Br₂ ↔ 2COBr₂

A mixture of 0.500 mol of carbon monoxide and 0.400 mol of bromine was placed into a rigid 1.00 L container and the system was allowed to come to equilibrium. The equlibrium concentration of COBr₂ was 0.223 M. What is the value of Kc for this reaction?

CO (g) + Br₂ (g) ↔ COBr₂ (g)

At 25 _oC, the equilibrium constant, Kc , for the reaction: B(g) + C(g) ↔ 2A(g) is 28.57. A mixture of 8.00 mol of B and 12.00 mol of C in a 20.0 L container is allowed to come to equilibirum. What is the equilibrium concentration of A?