Reaction 1) CBMP ? CA + phosphate ?G o = -12,300 cal/mole Reaction 2) ADP + phos

Question

Reaction 1) CBMP  ? CA + phosphate   ?Go   = -12,300 cal/mole

Reaction 2) ADP + phosphate  ? ATP    ?Go = +7,800 cal/mole

R = 1.987 cal/mole-degree

Standard temperature = 298o K

A. CBMP contains less free energy than (CA + phosphate)

B. ATP contains less free energy than (ADP + phosphate)

C. The energy which is released from the conversion of 1 mole of CBMP to   CA + phosphate (in reaction 1) is sufficient to drive the synthesis of 1 mole of ATP (in reaction 2)

I know that A and B are false and C is true, but my question is why? How do I know by looking at the information that A and B are fals and C is true?

A. CBMP contains less free energy than (CA + phosphate)

B. ATP contains less free energy than (ADP + phosphate)

C. The energy which is released from the conversion of 1 mole of CBMP to   CA + phosphate (in reaction 1) is sufficient to drive the synthesis of 1 mole of ATP (in reaction 2)

I know that A and B are false and C is true, but my question is why? How do I know by looking at the information that A and B are fals and C is true?

Explanation / Answer

A and B are false.

A. CBMP contains less free energy than (CA + phosphate) is false. According to the given information, CBMP contains more free energy than (CA + phosphate). See, bond breakage is exothermic. So, CBMP contains 12,300 cal/mole more energy than (CA + phosphate).

B. ATP contains less free energy than (ADP + phosphate) is false. Because bond formation is endothermic, (ADP + phosphate) utilise 7800 cal/mol energy to form ATP. So, ATP has 7800cal/mol more than (ADP+phosphate).

C is true. 12300cal/mole have been released out of which 7800cal/mole have been used up.

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