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Chapter 16: Problem 115

What are the catalysts in living cells called? Why are these biological catalysts necessary?

Short Answer

Expert verified
The catalysts in living cells are called enzymes. These biological catalysts are necessary because they speed up reactions, have specificity for certain reactions, regulate reactions based on cellular needs, and make processes more energy-efficient. Without enzymes, many vital biological processes would be too slow or impossible to occur, making life as we know it unfeasible.

Step by step solution

01

Answering the First Question

The catalysts present in living cells are known as enzymes.
02

Answering the Second Question

Enzymes, as biological catalysts, are necessary for a variety of reasons: 1. Speed up Reactions: Biological reactions naturally happen at a very slow rate. Enzymes speed these reactions up, ensuring that necessary biological functions happen in a timely manner. 2. Specificity: Each enzyme is specific to a certain reaction or a group of similar reactions. This ensures that reactions only occur when and where they're supposed to. 3. Regulating Reactions: Enzymes are not only catalysts but also regulate these reactions. They can increase or decrease the reaction rate as needed, allowing cells to respond to changes in the environment or the needs of the organism. 4. Energy Efficiency: By lowering the activation energy needed to commence a chemical reaction, enzymes make cellular processes more energy-efficient. Therefore, without enzymes, life as we know it would not exist, as many essential biological processes would occur too slowly or not at all.

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Most popular questions from this chapter

Why does an increase in temperature favor an increase in the speed of a reaction?

Magnesium fluoride dissolves in water to the extent of \(8.0 \times 10^{-2} \mathrm{g} / \mathrm{L}\) at \(25^{\circ} \mathrm{C} .\) Calculate the solubility of \(\mathrm{MgF}_{2}(s)\) in moles per liter, and calculate \(K_{\mathrm{sp}}\) for \(\mathrm{MgF}_{2}\) at \(25^{\circ} \mathrm{C}\).

What is the effect on the equilibrium position if an endothermic reaction is performed at a higher temperature? Does the net amount of product increase or decrease? Does the value of the equilibrium constant change if the temperature is increased?

Suppose that for the following reaction $$2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ it is determined that, at equilibrium at a particular temperature, the concentrations are as follows: \([\mathrm{NO}(g)] 8.1 \times 10^{-3} M,\left[\mathrm{H}_{2}(g)\right]=4.1 \times 10^{-5} M,\left[\mathrm{N}_{2}(g)\right]\) \(=5.3 \times 10^{-2} \mathrm{M}\) and \(\left[\mathrm{H}_{2} \mathrm{O}(g)\right]=2.9 \times 10^{-3} \mathrm{M} .\) Calculate the value of \(K\) for the reaction at this temperature.

Why does increasing the temperature for an exothermic process tend to favor the conversion of products back to reactants?
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