We find the following statement in a chemistry textbook: "At pH7.0 and 0.01 M Mg2+ ion, the standard free-energy change for ATP hydrolysis (ATP +
H20 -> ADP + Pi) is -28 kJ/mol." This means that-
1 mole of ADP and Pi in a one molar solution is lower in free energy by 28 kJ/mol than 1 mole of ATP and 1 mole of water under the given set of
conditions.
at any concentration of the 2 reactants and 2 products the difference of free energy between the reactants and products is 28 kJ/mol.
when the reaction reaches equilibrium, the free energy of ADP and Pi is lower by 28 kJ/mol than that of ATP and water.
when the reaction reaches equilibrium, the free energy of ADP and Pi is higher by 28 kJ/mol than that of ATP and water.
1 mole of ADP and Pi in a one molar solution is higher in free energy by 28 kJ/mol than 1 mole of ATP and 1 mole of water under the given set of
We Find The Following Statement In A Chemistry Textbook At Ph7 0 And 0 01 M Mg2 Ion The Standard Free Energy Change 1 (18.81 KiB) Viewed 59 times
QUESTION 21 We find the following statement in a chemistry textbook "At pH7.0 and 0.01 M Mg2+ ion, the standard free-energy change for ATP hydrolysis (ATP + H2O -> ADP.Pois 28 kl/mol. This means that 1 mole of ADP and Pi in a one molar solution is lower in free energy by 28 kJ/mol than 1 mole of ATP and 1 molo of water under the given set of conditions ut any concentration of the reactants and 2 products the difference of fros energy between the reactants and products is 28 kJ/mol. when the reaction reaches equilibrium, the free energy of ADP and Pl is lower by 28 kJ/mol than that of ATP and water when the reaction reaches oqulibrium, the free energy of ADP and Pi is higher by 28 kJ/mol than that of ATP and water 1 molo ot ADP and Prin a one molar solution is higher in free energy by 28 kamol than 1 mol of ATP and 1 mole of water under the given not of conditions
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