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In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g)+3H2(g)→2NH3(g) ΔG∘ at 298K for this reaction is −33.3kJ/mol. The value of ΔG at 298K for a reaction mixture that consists of 1.3atmN2, 1.4atmH2, and 0.78atmNH3 is ________ kJ/mol. In the Haber process, ammonia is synthesized from nitrogen and hydrogen: at for this reaction is . The value of at for a reaction mixture that consists of , , and is ________ . −4.42×103 −76.6 −37.7 −5.7 −2.13 × 103

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Answer:

Δ[tex]G=-37.7kJ/mol[/tex]

Explanation:

Hello,

Gibbs free energy for this reaction is defined as:

Δ[tex]G=[/tex]Δ[tex]G^0+RTln(Q)[/tex]

Now, [tex]Q[/tex] is computed via the law of mass action:

[tex]Q=\frac{P_{NH_3}^2}{P_{N_2}P_{H_2}^3} =\frac{0.78^2}{1.3*1.4^3}=0.17[/tex]

Finally:

Δ[tex]G=-33.3kJ/mol+298K*8.314x10^{-3}\frac{kJ}{mol*K}*ln(0.17)=-37.7kJ/mol[/tex]

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