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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 :

SEBASSANDINGO

Answer:

a. [tex]H_2+Cl_2 \rightleftharpoons 2HCl[/tex]

b. K = 192.9

c. Products are favored.

Explanation:

Hello!

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

[tex]H_2+Cl_2 \rightleftharpoons 2HCl[/tex]

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:

[tex]K=\frac{[HCl]^2}{[H_2][Cl_2]}[/tex]

Therefore, we plug in the data to obtain:

[tex]K=\frac{(0.0625)^2}{(0.00450)(0.00450)}\\\\K=192.9[/tex]

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

Best regards!

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