Question

1) Gaseous hydrogen bromide decomposes at elevated temperatures according to the following 10) equation: 2 HBr(g) H2(g) + Br2(g). At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr. What is the value of Kc at that temperature if the flask contains 0.104 mol of H2 at equilibrium?

2)In a 1.0 L vessel, at 698 K, 0.844 M H2 (g) and 0.844 M I2 (g) are combined. What is the 12) concentration of HI (g) at equilibrium? Kc = 54.3 at 698 K.

Hi, can someone please explain these as simple as possible thank you,