This question has multiple parts. Work all the parts to get the most points. Con

Question

This question has multiple parts. Work all the parts to get the most points. Consider the three hypothetical reactions shown below.

In all cases, the value of G° = -10.00 kJ mol-1 for each reaction. The concentration for each species in each reaction is given next to the reaction. You may assume that T = 25.0 °C.

What is the value of G (not G°) for each of these reactions under these conditions? Reaction 1: A B + C

[A] = 5.00 mM

[B] = 5.00 mM

[C] = 1.00 mM

G = kJ mol-1

Reaction 2: D + E F

[D] = 5.00 mM

[E] = 10.0 mM

[F] = 1.00 mM

G = kJ mol-1

Reaction 3: G H

[G] = 10.0 mM

[H] = 5.00 mM

G = kJ mol-1

Explanation / Answer

dG° = -10 = -10000

dG = dG° + RT*ln(Q)

a)

Q = [B][C]/[A]

Q = (5*10^-3)(1*10^-3)/(5*10^-3) = 0.001

dG = dG° + RT*ln(Q)

dG = -10000 + (8.314*298)*ln(0.001)

dG = -27114.46 J/mol

dG = -27.114 kJ/mol

b)

Q = [F]/([D][E])

Q = (10^-3)/((5*10^-3)(10*10^-3))

Q = 20

dG = dG° + RT*ln(Q)

dG = -10000 + (8.314*298)*ln(20)

dG = -2577.85

dG = -2.57 kJ/mol

c)

Q = [H]/[G]

Q = 5/10 = 0.5

dG = dG° + RT*ln(Q)

dG = -10000 + (8.314*298)*ln(0.5)

dG = -11717.32 J/mol

dG = -11.7 kJ/mol

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