Two (2.00) moles of NO, one (1.00) mole of Cl₂ , and two (2.00) moles of NOCl are placed in a 1.00 liter flask. If K c for 2 NO (g) + Cl₂ (g) 2 NOCl (g) is 2.72 at this temperature, what occurs in the flask as equilibrium is approached?

Question

Two (2.00) moles of NO, one (1.00) mole of Cl₂ , and two (2.00) moles of NOCl are placed in a 1.00 liter flask. If K c for 2 NO (g) + Cl₂ (g)  2 NOCl (g) is 2.72 at this temperature, what occurs in the flask as equilibrium is approached?

Quizplus · Accepted Answer

Since the initial amounts of reactants and products were given, we can use the reaction quotient Qc to determine which direction the reaction will proceed to reach equilibrium.

Qc = [NOCl]² / [NO]²[Cl₂]

When plugging in the initial concentrations, we get:

Qc = (2.00 M)² / (2.00 M)²(1.00 M) = 2.00

Comparing Qc and Kc, we see that Qc < Kc, indicating that the reaction will proceed forward to reach equilibrium.

As the forward reaction occurs, NO and Cl₂ will be consumed while NOCl will be produced, thus increasing the concentration of NOCl. Therefore, the answer is D - the [NOCl] increases.

Two (200) Moles of NO, One (1