The standard free energy change, delta f G, for the formation of NO (g) from its elements is +86.58 kJ/mol at 25 degrees C. Calculate Kp at this temperature for the equilibrium

1/2 N2(g) + 1/2 O2(g) = NO(g)
Comment on the sign of delta G and the magnitude of Kp.

1 answer

1/2N2 + 1/2O2 --> NO
dGfo = +86.58 kJ/mol.

dG = -RTlnKp
86,580 = -8.314*298*lnK
K = approx 10^-16
With a + sign for dG and the VERY small Kp, it is obvious that not much N2 will react with O2 to produce NO.
Similar Questions
  1. I have to find delta G from a problem.Not the standard free energy, from the change in engery. So this delta G does not have the
    1. answers icon 1 answer
    1. answers icon 1 answer
  2. N2(g)+3F2 yields 2Nf3(g)Delta H(degree)298=-264KJ mol-1;Delta S(degree)298=-278J K-1 mol-1 The following questions relate to the
    1. answers icon 0 answers
  3. Use standard enthalpies of formation to determine ΔHorxnfor:3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) -133.5 = Delta H Find the
    1. answers icon 1 answer
more similar questions