Question

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

Answer 1

Δ
`G=-37.7kJ/mol`

Step-by-step explanation:

Hello,

Gibbs free energy for this reaction is defined as:

Δ
`G=`Δ
`G^0+RTln(Q)`

Now,
`Q` is computed via the law of mass action:

`Q=(P_(NH_3)^2)/(P_(N_2)P_(H_2)^3) =(0.78^2)/(1.3*1.4^3)=0.17`

Finally:

Δ
`G=-33.3kJ/mol+298K*8.314x10^(-3)(kJ)/(mol*K)*ln(0.17)=-37.7kJ/mol`

Best regards.