Consider the chemical system CO + Cl 2 COCl 2 ;K = 4.6 $\times$ 10 9 L/mol. -If the concentration of the product were to double,what would happen to the equilibrium constant?

The equilibrium constant only changes with a change in temperature or pressure, not with changes in concentration. Therefore, doubling the concentration of the product will not change the value of the equilibrium constant.

Consider the chemical system CO + Cl 2 COCl 2 ;K = 4.6 $\times$ 10 9 L/mol. -If the concentration of the product were to double,what would happen to the equilibrium constant?

The equilibrium constant only changes with a change in temperature or pressure, not with changes in concentration. Therefore, doubling the concentration of the product will not change the value of the equilibrium constant.

Solved

Consider the Chemical System CO + Cl₂ COCl₂;K = $\times$

Question 9

Multiple Choice

Consider the chemical system CO + Cl₂ $Consider the chemical system CO + Cl2 COCl2;K = 4.6 \times 109 L/mol. -If the concentration of the product were to double,what would happen to the equilibrium constant? A) It would double its value. B) It would become half its current value. C) It would quadruple its value. D) It would not change its value. E) It would depend on the initial conditions of the product.$ COCl₂;K = 4.6 $\times$ 10⁹ L/mol.
-If the concentration of the product were to double,what would happen to the equilibrium constant?

A) It would double its value.
B) It would become half its current value.
C) It would quadruple its value.
D) It would not change its value.
E) It would depend on the initial conditions of the product.

Correct Answer: