Question
One of the important reactions in living cells from which the organism draws energy is the reaction of adenosine triphosphate (ATP) with water to give adenosine diphosphate (ADP) and free phosphate ion.$$\mathrm{ATP}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{ADP}+\mathrm{PO}_{4}^{3-}$$The value of $\Delta G_{310}^{\circ}$ for this reaction at $37^{\circ} \mathrm{C}$ (normal human body temperature) is $-33 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Calculate the value of the equilibrium constant for the reaction at this temperature.
Step 1
We do this by multiplying by 1000, as there are 1000 joules in a kilojoule. This gives us $\Delta G_{310}^{\circ} = -33 \times 1000 = -33000 \, \text{J mol}^{-1}$. Show more…
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Adenosine triphosphate (ATP) is a compound that provides energy for biomechanical reactions in the body when it undergoes hydrolysis. For the hydrolysis of ATP at 37 °C (normal body temperature), ΔG°r = -20.0 kJ⋅mol⁻¹ and ΔS°r = +34.0 J⋅K⁻¹⋅mol⁻¹. Assuming that these quantities are independent of temperature, calculate the temperature above which the equilibrium constant for the hydrolysis of ATP becomes greater than one.
Energy is stored in the body in adenosine triphosphate, ATP, which is formed by the reaction between adenosine diphosphate, ADP, and dihydrogen phosphate ions. $\mathrm{ADP}^{3-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{PO}_{4}^{2-}(\mathrm{aq}) \longrightarrow \mathrm{ATP}^{i-}(\mathrm{aq})+\mathrm{H}_{2} 0(\ell)$ $\Delta H^{\circ}=38 \mathrm{~kJ}$ Is the reaction endothermic or exothermic?
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