🤓 Based on our data, we think this question is relevant for Professor Hirsh's class at TCNJ.
H2(g) + I2(g) ⇌ 2 HI(g) K = 1.00 x 102
Step 1: Calculate the concentrations of the reactants and products.
[H2] = 1.00 M
[I2] = 1.00 M
[HI] = 1.00 M
Step 2: Calculate the reaction quotient.
Q = 1.00
Q < K → the reaction shifts in the forward direction to reach equilibrium
Step 3: Construct an ICE chart for the equilibrium reaction.
Step 4: Calculate the change (x) in the reaction using the equilibrium constant.
At a particular temperature, K = 1.00 x 102 for the reaction
H2(g) + I2(g) ⇌ 2HI(g)
In an experiment, 1.00 mole of H2, 1.00 mole of I2, and 1.00 mole of HI are introduced into a 1.00-L container. Calculate the concentrations of all species when equilibrium is reached.