# Problem: At a certain temperature, the equilibrium constant, K c, for the reaction Cl2(g) ⇌ 2Cl(g) is 5.92 x 104. A. If 2.77 g of Cl 2 are placed in a 2.50 L flask at this temperature, what are the equilibrium concentrations of Cl2 and Cl? B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 4.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl2 and Cl? C. Following the establishment of equilibrium in part A, the volume of the flask is instead suddenly decreased to 1.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl2 and Cl?

🤓 Based on our data, we think this question is relevant for Professor Du's class at UGA.

###### Problem Details

At a certain temperature, the equilibrium constant, K c, for the reaction

Cl2(g) ⇌ 2Cl(g)

is 5.92 x 104

A. If 2.77 g of Cl 2 are placed in a 2.50 L flask at this temperature, what are the equilibrium concentrations of Cl2 and Cl?

B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 4.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl2 and Cl?

C. Following the establishment of equilibrium in part A, the volume of the flask is instead suddenly decreased to 1.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl2 and Cl?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Le Chatelier's Principle concept. You can view video lessons to learn Le Chatelier's Principle . Or if you need more Le Chatelier's Principle practice, you can also practice Le Chatelier's Principle practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Du's class at UGA.