Question
Understanding the Energetics of the Glycogen Synthase Reaction (Integrates with Chapter 3 .) Suggest an explanation for the exergonic nature of the glycogen synthase reaction $\left(\Delta G^{\circ}=\right.$ $-13.3 \mathrm{kJ} / \mathrm{mol}$ ). Consult Chapter 3 to review the energetics of high-energy phosphate compounds if necessary.
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3 kJ/mol, we need to break down the process and relate it to the concepts of energetics, particularly focusing on high-energy phosphate compounds as mentioned. Here's how we can approach this: ### Show more…
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Explain why the glycogen phosphorylase reaction $\left(\Delta G^{\circ \prime}=\right.$ $3.1 \mathrm{kJ} \cdot \mathrm{mol}^{-1}$ ) is exergonic in the cell.
In biochemical reactions* the phosphorylation of amino acids is an important step. Consider the following two reactions and determine whether the phosphorylation of arginine with ATP is spontaneous. $$\mathrm{ATP}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{ADP}+\mathrm{P} \quad \Delta_{\mathrm{r}} G^{\circ \prime}=-31.5 \mathrm{kJ} \mathrm{mol}^{-1}$$ $$\begin{array}{l} \text { arginine }+\mathrm{P} \longrightarrow \text { phosphorarginine }+\mathrm{H}_{2} \mathrm{O} \\ \qquad \Delta_{\mathrm{r}} G^{\circ \prime}=33.2 \mathrm{kJ} \mathrm{mol}^{-1} \end{array}$$
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