Wednesday
March 29, 2017

Post a New Question

Posted by on .

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 bar for all species. For the reaction
C2H6(g)+H2(g)---->2CH4
the standard change in Gibbs free energy is ΔG° = -32.8 kJ/mol. What is ΔG for this reaction at 298 K when the partial pressures are
P(C2H6)=0.500bar, P(H2)=0.500bar, and P(CH4)=0.850bar
dG=____kj/mol

  • Chemistry - ,

    dG = dGo + RTlnQ

  • Chemistry - ,

    how do you find lnQ?

  • Chemistry - ,

    Q is the same form as K; i.e., concentrations in M of products over concentrations in M of reactants and raise each reagent to the power shown by the coefficients. In this case, you're dealing with pressures so it's partial pressure instead of concentrations. In other words make it look like a Kp expression. For example,
    A(g) + 2B(g) ==> 3C(g) you would have
    Q = pC^3/pA*p^B^2

  • Chemistry - ,

    Ok thanks a bunch!

Answer This Question

First Name:
School Subject:
Answer:

Related Questions

More Related Questions

Post a New Question