Consider the reaction A(g) ⇌ 2B(g)where K_p = 4.1 at 25°C.If 0.75 atm A(g)and 1.5 atm B(g)are initially present in a 1.0 L flask at 25°C,what change in partial pressures (if any)will occur in time?

Question

Quizplus · Accepted Answer

The equilibrium constant, K, shows that the reaction favors the products, 2B(g), over the reactant, A(g). Initially, there is more B(g) present than A(g). As the reaction proceeds, some of the A(g) will react to form more B(g), causing the partial pressure of A(g) to decrease and the partial pressure of B(g) to increase. Therefore, choice B is the correct answer.

Consider the Reaction A(g) ⇌ 2B(g)where Kp = 4

Consider the Reaction A(g) ⇌ 2B(g)where K_p = 4