Consider the following reaction at a certain temperature: PCl₅(g) PCl₃(g) + Cl₂(g)
K_c = 0.100
At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₃(g) and Cl₂(g) is added,what is the equilibrium concentration of PCl₅(g) ?

Question

Consider the following reaction at a certain temperature: PCl₅(g)

Consider the following reaction at a certain temperature: PCl<sub>5</sub>(g) PCl<sub>3</sub>(g) + Cl<sub>2</sub>(g) K<sub>c</sub> = 0.100 At equilibrium,[PCl<sub>5</sub>] = 2.00 M and [PCl<sub>3</sub>] = [Cl<sub>2</sub>] = 1.00 M.If suddenly 1.00 M PCl<sub>3</sub>(g) and Cl<sub>2</sub>(g) is added,what is the equilibrium concentration of PCl<sub>5</sub>(g) ? A) essentially 4.00 M B) 0.58 M C) 2.58 M D) 3.42 M E) 1.42 M

PCl₃(g) + Cl₂(g)
K_c = 0.100
At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₃(g) and Cl₂(g) is added,what is the equilibrium concentration of PCl₅(g) ?

Quizplus · Accepted Answer

The Answer of Consider the following reaction at a certain temperature: PCl₅(g) PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₃(g)and Cl₂(g)is added,what is the equilibrium concentration of PCl₅(g)?

Consider the Following Reaction at a Certain Temperature: PCl5(g)

Consider the Following Reaction at a Certain Temperature: PCl₅(g)