. Calculate the AG and Keg values for the reaction shown below: FADH2 +2 cyt.c-F
ID: 1034347 • Letter: #
Question
. Calculate the AG and Keg values for the reaction shown below: FADH2 +2 cyt.c-Fe3 FAD +2 cyt.c-Fe2 2H Standard oxidation/reduction potentials are: FAD/FADH E0.18 102 Faraday constant is; 23,063 cal/V E'+0.25 V cyt.c Fe/cyt.c Fe AG°" is: cal/mol b 6,560 cal/mol c. -5,650 cal/mol d -8,970 cal/mol e. -19,834 cal/mol K'eq is: a. 1.2X10-14 b. 3.56 x 1017 ?. 2.67 x 106 d. 3.46 x 1014 e. 3.20x10 13 A solution of 0.2 M dehydroascorbate and 0.2 M ascorbate (Eo0.06 V) was with an equal volume of a solution containing 0.01 M acetaldehyde and 0.01 M 1 (Eo__ 0.163 V) at 25°C and pH 7. Calculate the ?E?' for the possible n. a. - 0.103 b. +0.223 c. 0.223 d. +0.111 e. - 0.111 The Eo of the 2H* +2 e- H2 half reaction is arbitrarily set at zero. Calculate at pH 8. 0,378 V b. -0.286 V c. 0.143 V d.-0.143 V e. 0.472 V ulate ?pH across mitochondrial membrane driving the synthesis of ATP at temp. nder standard conditions. Assume ?Gor for ATP-7,700 cal/mole. 2 b. 3.25 c, 2.06 d. 1.08 e, 4.07
Explanation / Answer
1.
E0cell = E0right - E0left = + 0.25 - ( - 0.18 ) = 0.43 V
Relation between deltaG0 and E0cell is given by,
DeltaG0 = - n F E0cell = - 2 * 23063 * 0.43 = - 19834 cal/mol
So, the answer is (e)
Relation between deltaG0 and Keq is given by,
DeltaG0 = - R T lnK
- 19834 = - 1.987 * 298.15 * lnK
lnK = 33.48
K = 3.46 * 1014
So the anwer is (d)
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