Problem: At a particular temperature, K = 1.00 x 102 for the reactionH2(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.

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FREE Expert Solution

H2(g) + I2(g) ⇌ 2 HI(g)          K = 1.00 x 102


Step 1: Calculate the concentrations of the reactants and products.

Recall molarity

Molarity (M) =molL

[H2]=1.00 mol1.00 L[H2]=1.00 molL

[H2] = 1.00 M

[I2] = 1.00 M

[HI] = 1.00 M


Step 2: Calculate the reaction quotient.

Q=productsreactants


Q=productsreactants

Q=[HI]2[H2][I2]Q=(1.00)2(1.00)(1.00)

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.

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Problem Details

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.