Calculate the equilibrium constant at 298 K for the reaction of formaldehyde (CH2O) with hydrogen gas using the following information. CH2O(g) + 2H2(g) LaTeX: \longleftrightarrow⟷ CH4(g) + H2O(g) LaTeX: \DeltaΔH°= –94.9 kJ; LaTeX: \DeltaΔS°= –224.2 J/K A. 1.92 B. 9.17 x 10-6 C. 2.07 x 1028 D. 1.10 x 105 E. 8.08 x 104 F. 3.98 x 1011 Group of answer choices

E. 8.08 x 10⁴.

Explanation:

Hello,

In this case, for the reaction:

We can compute the Gibbs free energy of reaction via:

Since both the entropy and enthalpy of reaction are given at 298 K (standard temperature), therefore:

Then, as the equilibrium constant is computed as:

We obtain:

For which the answer is E. 8.08 x 10⁴.

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practical process described pest part of scientific investigation.

because practical knowledge is powerful then therotical knowledge.

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.