#Question id: 73
#Biochemistry
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
#Biochemistry
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: 75
#Biochemistry
The experimental approach taken in current biological investigations presumes that ________.
#Question id: 76
#Biochemistry
Which of the following illustrations is not a structural isomer of an organic compound with the molecular formula C6H14? For clarity, only the carbon skeletons are shown; hydrogen atoms that would be attached to the carbons have been omitted.
#Question id: 77
#Biochemistry
Which of the pairs of molecular structures shown depict enantiomers (enantiomeric forms) of the same molecule?
#Question id: 78
#Biochemistry
Which is true about naturally occurring monosaccharides?