An experimenter places the following concentrations of gases in a closed container: [NOBr] = 7.13 × 10^2 M, [NO] = 1.58 × 10^2 M, [Br₂] = 1.29 × 10^2 M. These gases then react:

2NOBr(g) ⇌ 2NO(g) + Br₂(g)

At the temperature of the reaction, the equilibrium constant K_c is 3.07 × 10^4. Calculate the reaction quotient, Q_c, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium.

a. Q_c = 6.33 × 10^4; the concentration of NOBr decreases

b. Q_c = 6.33 × 10^4; the concentration of NOBr increases

c. Q_c = 1.58 × 10⁴; the concentration of NOBr increases

d. Q_c = 4.65 × 10^4; the concentration of NOBr decreases

e. Q_c = 4.65 × 10^4; the concentration of NOBr increases