Question

Also determine how many moles of H2O2 have reacted with iodide at the instant:

a) The rate of the reaction equals zero.
b) The equilibrium is reached.
c) The concentration of iodide is constant.
d) The concentration of H2O2 is constant.

Answer 1

The equilibrium concentrations of H₂, I₂, and HI can be calculated using the equilibrium constant expression and the initial concentrations of the reactants.

Step-by-step explanation:

The equilibrium concentrations of H₂, I₂, and HI can be calculated using the equilibrium constant expression and the initial concentrations of the reactants.

Given:

• Initial concentration of H₂ = 1.00 moles/L
• Initial concentration of I₂ = 2.00 moles/L
• Equilibrium constant (K) = 50.5

To find the equilibrium concentrations:

1. Let x be the change in concentration of HI
2. Using the stoichiometry of the reaction, the change in concentration of H₂ and I₂ can be expressed as -2x and -2x, respectively
3. Write the equilibrium expression: K = [HI]2/([H₂][I₂])
4. Substitute the equilibrium concentrations into the equilibrium expression and solve for x
5. The equilibrium concentrations of H₂, I₂, and HI are then: [H₂] = 1.00 - 2x, [I₂] = 2.00 - 2x, and [HI] = x

Substituting these values into the expression for K will give you the equilibrium concentrations of H₂, I₂, and HI in moles/L.