Question

At equilibrium at 2500K, [HCl]=0.0625M and [H2]=[Cl2]=0.00450M for the reaction H2+Cl2 ⇌ HCl.

a. Determine the balanced equation and write the equilibrium expression
b. Determine the K eq
c. Will this process favor the reactants or products at equilibrium?

Answer 1

The balanced equation for the given reaction is H2 + Cl2 ⇌ 2HCl. The equilibrium expression for this reaction is K_eq = [HCl]^2 / ([H2][Cl2]). Given the concentrations at equilibrium, we can calculate the equilibrium constant as 312.5. This process favors the products (HCl) at equilibrium.

Step-by-step explanation:

In this reaction, H2 and Cl2 react to form 2HCl, with a balanced equation:

H2 + Cl2 ⇌ 2HCl

The equilibrium expression for this reaction is given by:

Keq = [HCl]2 / ([H2][Cl2])

Given the concentrations at equilibrium ([HCl] = 0.0625M and [H2] = [Cl2] = 0.00450M), we can substitute these values into the equilibrium expression to calculate the equilibrium constant:

Keq = (0.0625)2 / (0.00450)(0.00450) = 312.5

The equilibrium constant, Keq, is greater than 1, indicating that the process favors the products (HCl) at equilibrium.

Answer 2

a.
`H_2+Cl_2 \rightleftharpoons 2HCl`

b. K = 192.9

c. Products are favored.

Step-by-step explanation:

Hello!

a. In this case, according to the unbalanced chemical reaction we need to balance HCl as shown below:

`H_2+Cl_2 \rightleftharpoons 2HCl`

In order to reach 2 hydrogen and chlorine atoms at both sides.

b. Here, given the concentrations at equilibrium and the following equilibrium expression, we have:

`K=([HCl]^2)/([H_2][Cl_2])`

Therefore, we plug in the data to obtain:

`K=((0.0625)^2)/((0.00450)(0.00450))\\\\K=192.9`

c. Finally, we infer that since K>>1 the forward reaction towards products is favored.

Best regards!