BIOCHEMISTRY
BIOCHEMISTRY
9th Edition
ISBN: 2818440090622
Author: BERG
Publisher: MAC HIGHER
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Chapter 15, Problem 24P
Interpretation Introduction

Interpretation:

The ratio of the reactants to the products under the intracellular as well as in the equilibrium conditions is to be stated. The way by which reaction becomes exergonic under intracellular condition and becomes endergonic under the standard condition is to be stated.

Concept introduction:

A thermodynamic potential that is utilized in the calculation of the highest reversible function taking place in the thermodynamic system at the constant value pressure and temperature is known as Gibbs-free energy. It is denoted by ΔG°.

Expert Solution & Answer
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Answer to Problem 24P

The ratio of the reactants to the products under the intracellular condition is. 3.99×105 and under the equilibrium condition is 6.742×105.

Explanation of Solution

The reaction that is catalysis by the enzyme aldolase in the glycolytic pathway is given as follows.

Fructose1,6bisphosphatemdihydroxyacetatephosphate+glceraldehyde3phosphate

The value of standard ΔG°' for this given reaction is +23.8kJmol1 or +5.7kcalmol1.

The value of ΔG inside the cell is 1.3kJmol1 or 0.3kcalmol1.

The value of universal gas constant is 8.315×103kJmol1K1.

The standard temperature is 25°C.

The conversion of degrees Celsius into Kelvin is done as,

0°C=273K

Thus, the given temperature becomes,

25°C=25+273K=298K

The value of standard ΔG°' under equilibrium condition for the given reaction is calculated by the expression as follows.

ΔG°'=RTlnKeq=RTln[Products][Reactants](1)

Where,

  • R is the universal gas constant.
  • T is the temperature.
  • Keq is the equilibrium constant.

Substitute the values of universal gas constant, temperature and value of standard ΔG°' for this given reaction in equation (1).

+23.8kJmol1=8.315×103kJmol1K1×298K×ln[Products][Reactants]+23.8kJmol1=2.478kJmol1×ln[Products][Reactants][Products][Reactants]=e9.6045=6.742×105

Thus, the ratio of the reactants to the products under equilibrium condition is 6.742×105.

The value of ΔG under intracellular condition for the given reaction is calculated by the expression as follows.

ΔG=ΔG°'+RTlnK=ΔG°'+RTln[Products][Reactants](2)

Where,

  • ΔG is the actual free energy change.
  • ΔG°' is the standard free-energy change.
  • R is the universal gas constant.
  • T is the temperature.

Substitute the values of universal gas constant, temperature and value of ΔG for this given reaction in equation (2).

1.3kJmol1=23.8kJmol1+8.315×103kJmol1K1×298K×ln[Products][Reactants]1.3kJ mol 123.8kJ mol 18.315× 10 3kJ mol 1K 1×298K=ln[Products][Reactants][Products][Reactants]=e10.13=3.99×105

Thus, the ratio of the reactants to the products under equilibrium condition is 6.742×105 and under the intracellular condition is. 3.99×105.

Thus, according to the ratio of products to the reactants, if this ratio is kept lower than the equilibrium value then this given reaction, which is endergonic under the standard conditions, is able to convert itself into exergonic.

This type of transformation is obtained only if the product of the given reaction is used in some other reaction after its immediate formation.

Conclusion

The ratio of the reactants to the products under the intracellular condition is. 3.99×105 and under the equilibrium condition is 6.742×105.

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