Consider the hydrolysis of ATP: ATP(aq) + H2O(l) → ADP(aq) + Pi(aq). This reaction has ΔH°= −24.3 kJ/mol and ΔS°= +21.6 J/mol-K. The actual concentrations of ATP, ADP, and Pi are not 1 M in a biological cell. How much energy can the conversion of ATP to ADP supply when it occurs at physiological conditions in E. coli where the temperature is 37°C and the approximate concentrations are ATP = 11.2 mM, ADP = 1.52 mM, Pi = 20.0 mM? Enter your answer to three significant figures in units of kJ. Include the sign.
Sol.
Reaction :
ATP(aq) + H2O(l) -----> ADP(aq) + Pi(aq)
As Standard change in enthalpy = deltaH° = - 24.3 KJ / mol
standard change in entropy = deltaS° = 21.6 J / K mol
= 21.6 / 1000 KJ / K mol = 0.0216 KJ / K mol
Temperature = T = 37°C = 37 + 273.15 K = 310.15 K
So , Standard change in free energy
= deltaG° = deltaH° - T × deltaS°
= ( - 24.3 KJ / mol ) - 310.15 K × 0.0216 KJ / K mol
= - 30.99924 KJ / mol
Now , [ADP] = 1.52 mM = 1.52 × 10-3 M
[Pi] = 20 mM = 20 × 10-3 M
[ATP] = 11.2 mM = 11.2 × 10-3 M
Reaction Quotient = Q
= [ADP] [Pi] / [ATP]
= 1.52 × 10-3 × 20 × 10-3 / ( 11.2 × 10-3 )
= 0.0027142857
Gas constant = R = 0.008314 KJ / K mol
Therefore , Change in free energy
= deltaG = deltaG° + RTln(Q)
= - 30.99924 KJ / mol + 0.008314 KJ / K mol × 310.15 K × ln ( 0.0027142857 )
= - 46.2 KJ / mol
Therefore , - 46.2 KJ of energy the conversion supply
Consider the hydrolysis of ATP: ATP(aq) + H2O(l) → ADP(aq) + Pi(aq). This reaction has ΔH°=...
Question 11 1 pts Consider the hydrolysis of ATP: ATP(aq) + H2O(1) - ADP(aq) + P(aq). This reaction has AH°= -24.3 kJ/mol and AS - +21.6 J/mol-K. The actual concentrations of ATP, ADP, and Pi are not 1 Min a biological cell. How much energy can the conversion of ATP to ADP supply when it occurs at physiological conditions in E.coli where the temperature is 37°C and the approximate concentrations are ATP - 14.8 mM, ADP - 3.65 MM, P,...
ATP + H2O <---> ADP + Pi Calculate the ΔG for ATP hydrolysis when the concentrations of ATP, ADP, and Pi are all 1M R = 1.98 x 10-3 T = 310 kelvin ΔGº = -30.5 kJ/mol
For the hydrolysis of ATP to ADP + Pi (AGº'=-30.5kJ/mol) what is AG'when [ATP], [ADP], and [Pi] are 8, 1, and 8 mM, respectively (use RT=2.48 kJ/mol). O Select one: A. -30.5 kJ/mol x O B.-17.1 kJ/mol C. -47.6 kJ/mol D. 13.4 kJ/mol O
The value of the standard free energy (∆G°’) for the hydrolysis of ATP (ATP + H2O -> ADP + Pi) is relatively difficult to determine because of the small concentration of ATP remaining at equilibrium. The value can be determined from the equilibrium constant of two related chemical reactions. Glucose-6-phosphate + H2O -> glucose + Pi ; k’eq = 270 ATP + glucose -> ADP + glucose-6-phosphate ; K’eq = 890 From this information, calculate the standard free energy of...
The first step in the metabolic breakdown of glucose is its phosphorylation to G6P: glucose(aq)+ATP(aq)→G6P(aq)+ADP(aq)+H+(aq)glucose(aq)+ATP(aq)→G6P(aq)+ADP(aq)+H+(aq) The standard reaction Gibbs energy for the reaction isΔGoΔGo= -34 kJ/mol at 37°C A. Calculate the biological standard reaction GIbbs energy for the reaction at 37°C. B. Calculate the equilibrium constant of the reaction in the thermodynamic standard (KeqKeq) at 37°C. Use 2 significant figures. c, Calculate the equilibrium constant of the reaction in the biological standard (K′eqKeq′) at 37°C. Use 2 significant figures.
We have seen all term that cells use the hydrolysis of high energy phosphate from ATP to make metabolic reactions thermodynamically favorable. Whereas most enzymes that utilize ATP hydrolyze between the b and g phosphates (yielding ADP + Pi), some enzymes hydrolyze ATP between the a and b phosphates (yielding AMP and PPi). ∆G°’ of phosphate hydrolysis is -31 kJ/mol for ATP + H2O --> ADP + Pi, and ∆G°’ of phosphate hydrolysis is -46.5 kJ/mol for ATP + H2O...
ATP(aq) +H20(l) >>>ADP(aq) + HPO4^2- for which ΔG°rxn = –30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of ΔGrxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.60 mM, and [HPO42–] = 5.0 mM.
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H2O(l) —— ADP(aq) + HPO2 (aq) for which AGix = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGrxn in a biological cell in which [ATP] = 5.0 mm, (ADP) = 0.20 mM, and [HPO2-) = 5.0 mM. AGxn= kJ/mol...
Part F Calculate the energy available from hydrolysis of ATP if the ATP/ADP ratio is 5:1, the inorganic phosphate concentration is 50 mM and the temperature is 37°C? (Assume AG' = -7.3 kcal/mol for ATP hydrolysis.) Express your answer as an integer. AG' = -10100 cal/mol Submi Previous Answers Correct Part 1 Calculate the energy needed to synthesize ATP if the temperature is 25°C, and the ATP, ADP and inorganic phosphate concentrations are as in part F? (Assume AG' =-7.3...
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction..... Thank you!!! A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H2O(1) ADP(aq) + HPO2 (aq) in a biological...