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Chapter 14: Problem 51

A certain reaction is known to proceed slowly at room temperature. Is it possible to make the reaction proceed at a faster rate without changing the temperature?

Short Answer

Expert verified
Yes, it is possible to make the reaction proceed at a faster rate without changing the temperature. This can be achieved by introducing a catalyst into the reaction or by influencing other factors such as increasing the concentration of reactants, the pressure (for gases), or the surface area of a solid reactant.

Step by step solution

01

Understanding the Basics

Before answering the question, it's important to understand that in Chemistry, the rate of a reaction can be altered without necessarily changing the temperature. This is possible by influencing other factors that could affect the reaction rate.
02

Introduce a Catalyst

A catalyst is a substance that can expedite a reaction without being used up in the process. It accomplishes this by reducing the amount of energy required for the reaction to occur, facilitating a faster reaction rate.
03

Other Possible Ways

Adding a catalyst isn't the only way to make a reaction proceed faster at a constant temperature. Other ways include increasing the concentration of reactants, the pressure (for gases), or the surface area of a solid reactant.

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Most popular questions from this chapter

Use the Arrhenius equation to show why the rate constant of a reaction (a) decreases with increasing activation energy and (b) increases with increasing temperature.

Consider the following elementary steps for a consecutive reaction $$ \mathrm{A} \stackrel{k_{1}}{\longrightarrow} \mathrm{B} \stackrel{k_{2}}{\longrightarrow} \mathrm{C} $$ (a) Write an expression for the rate of change of \(\mathrm{B}\). (b) Derive an expression for the concentration of \(\mathrm{B}\) under steady- state conditions; that is, when \(\mathrm{B}\) is decomposing to \(\mathrm{C}\) at the same rate as it is formed from \(\mathrm{A}\).

Explain why termolecular reactions are rare.

The integrated rate law for the zero-order reaction \(\mathrm{A} \longrightarrow \mathrm{B}\) is \([\mathrm{A}]_{t}=[\mathrm{A}]_{0}-k t .\) (a) Sketch the follow- ing plots: (i) rate versus \([\mathrm{A}]_{t}\) and (ii) \([\mathrm{A}]_{t}\) versus \(t\). (b) Derive an expression for the half-life of the reaction. (c) Calculate the time in half-lives when the integrated rate law is no longer valid, that is, when \([\mathrm{A}]_{t}=0\)

For each of these pairs of reaction conditions, indicate which has the faster rate of formation of hydrogen gas: (a) sodium or potassium with water, (b) magnesium or iron with \(1.0 \mathrm{M} \mathrm{HCl}\), (c) magnesium rod or magnesium powder with \(1.0 \mathrm{M} \mathrm{HCl}\), (d) magnesium with \(0.10 M \mathrm{HCl}\) or magnesium with \(1.0 \mathrm{M} \mathrm{HCl}\).
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