#Question id: 72
#SCPH05 I Biotechnology
For the reaction catalyzed by the enzyme hexokinase: Glucose + ATP → glucose 6-phosphate + ADP the equilibrium constant, Keq, is 7.8 × 102. In living E. coli cells, [ATP] = 5 mM, [ADP] = 0.5 mM, [glucose] = 2 mM, and [glucose 6-phosphate] = 1 mM. Which of the following conclusions made on the basis of the above calculations is incorrect?
#Question id: 72
#SCPH06 I Botany
For the reaction catalyzed by the enzyme hexokinase: Glucose + ATP → glucose 6-phosphate + ADP the equilibrium constant, Keq, is 7.8 × 102. In living E. coli cells, [ATP] = 5 mM, [ADP] = 0.5 mM, [glucose] = 2 mM, and [glucose 6-phosphate] = 1 mM. Which of the following conclusions made on the basis of the above calculations is incorrect?
#Question id: 73
#SCPH05 I Biotechnology
Match the Variation of Reaction Spontaneity (Sign of ΔG) given in Column I with the Signs of ΔH and ΔS given in column II.
|
COLUMN I |
COLUMN II |
|
|
|
|
ΔH |
ΔS |
ΔG = ΔH – TΔS |
|
1. |
− |
+ |
a. The
reaction is both enthalpically and entropically opposed. It is nonspontaneous
(endergonic) at all temperatures. |
|
2. |
− |
− |
b. The
reaction is enthalpically opposed (endothermic) but entropically favored. It
is spontaneous only at temperatures above T = ΔH/ΔS. |
|
3. |
+ |
+ |
c. The
reaction is enthalpically favored but entropically opposed. It is spontaneous
only at temperatures below T = ΔH/ΔS. |
|
4. |
+ |
− |
d. The
reaction is both enthalpically favored (exothermic) and entropically favored.
It is spontaneous (exergonic) at all temperatures. |
#Question id: 73
#SCPH06 I Botany
Match the Variation of Reaction Spontaneity (Sign of ΔG) given in Column I with the Signs of ΔH and ΔS given in column II.
|
COLUMN I |
COLUMN II |
|
|
|
|
ΔH |
ΔS |
ΔG = ΔH – TΔS |
|
1. |
− |
+ |
a. The
reaction is both enthalpically and entropically opposed. It is nonspontaneous
(endergonic) at all temperatures. |
|
2. |
− |
− |
b. The
reaction is enthalpically opposed (endothermic) but entropically favored. It
is spontaneous only at temperatures above T = ΔH/ΔS. |
|
3. |
+ |
+ |
c. The
reaction is enthalpically favored but entropically opposed. It is spontaneous
only at temperatures below T = ΔH/ΔS. |
|
4. |
+ |
− |
d. The
reaction is both enthalpically favored (exothermic) and entropically favored.
It is spontaneous (exergonic) at all temperatures. |
#Question id: 74
#SCPH05 I Biotechnology
The enthalpy and entropy of the initial and final states of a reacting system are shown in the table. Calculate the change in free energy for the reaction when the temperature is 4°C.
#Question id: 74
#SCPH06 I Botany
The enthalpy and entropy of the initial and final states of a reacting system are shown in the table. Calculate the change in free energy for the reaction when the temperature is 4°C.