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Chapter 12: Problem 71

Why is it important that at least some of the spontaneous steps in glycolysis convert ADP to ATP?

Short Answer

Expert verified
Answer: Spontaneous steps in glycolysis are important for the conversion of ADP to ATP because they couple unfavorable reactions with favorable ones, allowing energy to be released through substrate-level phosphorylation. This process generates ATP, providing cells with the necessary energy to carry out essential processes and maintain homeostasis, thus contributing to the overall balance of cellular metabolism.

Step by step solution

01

Introduction to glycolysis

Glycolysis is a metabolic pathway that is involved in the breakdown of glucose, a six-carbon sugar molecule, to produce pyruvate, a three-carbon molecule. This pathway is crucial for providing cells with energy in the form of ATP, as well as generating key intermediates for other metabolic pathways.
02

Understanding ATP and ADP

Adenosine triphosphate (ATP) is a high-energy molecule that acts as the main currency of energy for cellular processes. On the other hand, adenosine diphosphate (ADP) is a lower-energy molecule generated when ATP loses a phosphate group. The conversion between ADP and ATP allows energy to be stored and released on demand to power various biological processes.
03

The role of spontaneous steps in glycolysis

In glycolysis, there are a few enzymatic reactions that are spontaneous, meaning they occur without input of external energy. These reactions play a crucial role in glycolysis, as they help "couple" unfavorable (higher-energy) reactions with favorable (lower-energy) ones. In the context of glycolysis, this means that certain spontaneous steps help to convert ADP to ATP.
04

Phosphorylated intermediates and energy yield

The spontaneous steps in glycolysis that couple the conversion of ADP to ATP occur through the reactions involving phosphorylated intermediates. As the phosphate groups are transferred, energy is released, and this energy is utilized to convert ADP to ATP in a process called substrate-level phosphorylation.
05

Importance of ADP to ATP conversion

The conversion of ADP to ATP during glycolysis is important because it ensures that cells have an adequate supply of energy to carry out essential processes and maintain homeostasis. This allows glycolysis to contribute to the overall energy balance of the cell, which is critical for its survival and functioning. In addition, by generating ATP, glycolysis also provides a source of energy for other metabolic pathways that rely on ATP as a primary energy source. In conclusion, spontaneous steps in glycolysis are important for the efficient conversion of ADP to ATP, which provides the necessary energy for cellular processes and contributes to the overall balance of cellular metabolism.

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Most popular questions from this chapter

Calculate the free-energy change for the dissolution in water of one mole of \(\mathrm{NaBr}\) and one mole of \(\mathrm{NaI}\) at \(298 \mathrm{K}\) from the values in the following table. $$\begin{array}{lcc}\hline & \Delta H_{\text {solution }}^{\circ}(\mathrm{k} J / \mathrm{mol}) & \Delta S_{\text {solution }}^{\circ}[J /(\mathrm{mol} \cdot \mathrm{K})] \\\\\text { NaBr } & -0.60 & 57 \\\\\hline \text { Nal } & -7.5 & 74 \\\\\hline\end{array}$$

Use the standard molar entropies in Appendix 4 to calculate the \(\Delta S^{\circ}\) value for each of the following reactions of sulfur compounds. a. \(\mathrm{H}_{2} \mathrm{S}(g)+\frac{3}{2} \mathrm{O}_{2}(g) \rightarrow \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{SO}_{2}(g)\) b. \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) c. \(\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) d. \(S(g)+O_{2}(g) \rightarrow S O_{2}(g)\).

Which of the following combinations of entropy changes for a process are mathematically possible? a. \(\Delta S_{\text {sys }}<0, \Delta S_{\text {surr }}>0, \Delta S_{\text {univ }}>0\) b. \(\Delta S_{\text {sys }}<0, \Delta S_{\text {surr }}<0, \Delta S_{\text {univ }}>0\) c. \(\Delta S_{\text {sys }}<0, \Delta S_{\text {surr }}>0, \Delta S_{\text {univ }}<0\)

Gas streams containing \(\mathrm{CO}_{2}\) are frequently passed through absorption tubes filled with \(\mathrm{CaO}(s),\) where the following reaction takes place to remove the \(\mathrm{CO}_{2}\) from the stream:$$\mathrm{CaO}(s)+\mathrm{CO}_{2}(g) \rightarrow \mathrm{CaCO}_{3}(s)$$. a. Use the data in Appendix 4 to calculate \(\Delta G^{\circ}\) at \(298 \mathrm{K}\) for this reaction. b. Is the reaction spontaneous at \(298 \mathrm{K} ?\) c. Calculate \(\Delta G\) for this reaction at \(1500 \mathrm{K},\) a typical temperature for a lime kiln. (Assume \(\Delta H\) and \(\Delta S\) do not change with temperature.) d. Is the reaction as written spontaneous at \(1500 \mathrm{K}\) ? e. In a lime kiln, calcium carbonate (in the form of oyster shells) is roasted to produce \(\mathrm{CaO}\) and \(\mathrm{CO}_{2} .\) Is this process spontaneous at the temperature of a kiln?

Adding sidewalk deicer (calcium chloride) to water causes the temperature of the water to increase. If solid \(\mathrm{CaCl}_{2}\) is the system, what are the signs of \(\Delta S_{\mathrm{sys}}\) and \(\Delta S_{\mathrm{surr}} ?\)
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