Question

HCl(g) can be made by the direct reaction of H2 and Cl2 in the presence of light. 3.00 g of H2 and 140 g Cl2 are mixed in a 10.00 L flask at 28.0 °C. What are the partial pressures of gases after the reaction has completed. Assume ideal behavior for all gases. Here is the data you'll need:

Temperature and volume remain constant at 28.0 °C
Wavelength of light needed for the reaction is 340 nm.​

Answer 1

To determine the equilibrium composition of a mixture of H2 and Cl2 at 47°C, the equilibrium constant Kc must be calculated using the concentrations of reactants and products at equilibrium.

Step-by-step explanation:

Given that H2(g) + Cl2(g) → 2HCl(g)

A mixture of 0.257 M H2 and 0.392 M Cl2 is allowed to equilibrate at 47°C. To determine the equilibrium composition of the mixture, we need to calculate the equilibrium constant Kc.

Equilibrium constant Kc is determined using the concentrations of reactants and products at equilibrium. In this case, [HCl]^2/([H2][Cl2]) = Kc. By substituting the given concentrations into the equation, we can find the equilibrium composition of the mixture.