Consider the three hypothetical reactions shown below. In all cases, the value o

Question

Consider the three hypothetical reactions shown below. In all cases, the value of delta G percent= 10.00kJ 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 delta G (not delta G percent) for each of these reactions under these conditions.

History Bookmarks Window Help 38% D T east.cengagenow.com ns shown below. In all cases, the value of G"-10.00 kJ mol-1 for OWLv2 | Onine seaching and learning resource from Cengage Lear Consider the three hypothetical reactions shown below. In all cases, the value of AG 10.00 kJ mol for each reaction. The concentration for species in each reaction is given next to the reaction. You may assume that T-25.0 °C what is the value of AG (not G*) for each of these reactions under these conditions? Reaction I B+C [A]-5.00 mM [B] 500. mM [C]-1.00 mMM AG- kJ mol Reaction 2: D+E [DI-50.0 mM [E]-1.00 mM . [F]-500. mf AG kJ mol Reaction 3: (G]- 500. mM [H] 5.00 mf AG kJ mol" Show Hint 7 8 9

Explanation / Answer

overall

dG = dG° + RT*ln(Q)

then

RXN1

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

Q = (0.5)(1*10^-3)/(5*10^-3) = 0.1

dG = dG° + RT*ln(Q)

dG = 10000 +8.314 *298 * ln(0.1)

dG = 4295.1 J/mol

dG = 4.29 kJ/mol

RXN 2

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

Q = (0.5)/((10^-3)(50*10^-3))

Q = 10000

dG = dG° + RT*ln(Q)

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

dG = 32819.2

dG = 32.8 kJ/mol

RXN3

Q = [H]/[G] = (5*10^-3)/(0.5) = 0.01

dG = dG° + RT*ln(Q)

dG = 10000 +8.314 *298 * ln(0.01)

dG = -1409.64 J/mol

dG = -1.41 kJ/mol

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