The oxidation of malate by NAD to form oxaloacetate is a highly endergonic reaction under standard conditions. AG" = +29 kJ mol-¹ (+7 kcal mol-¹) Malate + NAD+ oxaloacetate + NADH + H+ The reaction proceeds readily under physiological conditions. Why does the reaction proceed readily as written under physiological conditions? Endergonic reactions such as this occur spontaneously without the input of free energy. The steady-state concentrations of the products are low compared with those of the substrates. The reaction is pushed forward by the energetically favorable oxidation of fumarate to malate. The NADH produced during glycolysis drives the reaction in the direction of malate oxidation. Assuming an [NAD+ ]/[NADH] ratio of 8, a temperature of 25°C, and a pH of 7, what is the lowest [malate]/[oxaloacetate] ratio at which oxaloacetate can be formed from malate? [malate] [oxaloacetate] =

Biochemistry
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Chapter1: Biochemistry: An Evolving Science
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The oxidation of malate by NAD to form oxaloacetate is a highly endergonic reaction under standard conditions.
AG° = +29 kJ mol¯¹ (+7 kcal mol¯¹)
Malate + NAD+ = oxaloacetate + NADH + H+
The reaction proceeds readily under physiological conditions.
Why does the reaction proceed readily as written under physiological conditions?
Endergonic reactions such as this occur spontaneously without the input of free energy.
The steady-state concentrations of the products are low compared with those of the substrates.
The reaction is pushed forward by the energetically favorable oxidation of fumarate to malate.
O The NADH produced during glycolysis drives the reaction in the direction of malate oxidation.
Assuming an [NAD* ]/[NADH] ratio of 8, a temperature of 25°C, and a pH of 7, what is the lowest [malate]/[oxaloacetate] ratio
at which oxaloacetate can be formed from malate?
[malate]
[oxaloacetate]
=
Transcribed Image Text:T The oxidation of malate by NAD to form oxaloacetate is a highly endergonic reaction under standard conditions. AG° = +29 kJ mol¯¹ (+7 kcal mol¯¹) Malate + NAD+ = oxaloacetate + NADH + H+ The reaction proceeds readily under physiological conditions. Why does the reaction proceed readily as written under physiological conditions? Endergonic reactions such as this occur spontaneously without the input of free energy. The steady-state concentrations of the products are low compared with those of the substrates. The reaction is pushed forward by the energetically favorable oxidation of fumarate to malate. O The NADH produced during glycolysis drives the reaction in the direction of malate oxidation. Assuming an [NAD* ]/[NADH] ratio of 8, a temperature of 25°C, and a pH of 7, what is the lowest [malate]/[oxaloacetate] ratio at which oxaloacetate can be formed from malate? [malate] [oxaloacetate] =
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