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Chapter 13: Problem 62

Distinguish between homogeneous catalysis and heterogeneous catalysis. Describe three important industrial processes that utilize heterogeneous catalysis.

Short Answer

Expert verified
Homogeneous catalysis is when the catalyst and reactants share the same phase, while heterogeneous catalysis is when they are in different phases. Examples of industrial processes using heterogeneous catalysis include the Haber Process, the Ostwald process, and the Catalytic Cracking process in petroleum refining.

Step by step solution

01

Define Homogeneous Catalysis

Homogeneous catalysis refers to the process where the catalyst and the reactants are in the same phase or state of matter. This typically occurs when all are present in the same liquid or gas phase.
02

Define Heterogeneous Catalysis

Heterogeneous catalysis, on the other hand, is the process where the catalyst and the reactants are in different phases, i.e., they are physically different and separate. This is common when the catalyst is a solid and the reactants are either in liquid or gas phase.
03

Examples of Industrial Processes Utilizing Heterogeneous Catalysis

Heterogeneous catalysis is utilized in numerous industrial processes. Here are three examples:\n1. The Haber Process: In this process, nitrogen and hydrogen gases react over a solid iron catalyst to produce ammonia.\n2. The Ostwald process: This process uses a platinum catalyst to convert ammonia into nitric acid.\n3. The Catalytic Cracking process: In the refining of petroleum, a solid acid catalyst is used to break long-chain hydrocarbons into shorter, more useful fractions.

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Most popular questions from this chapter

At \(25^{\circ} \mathrm{C},\) the rate constant for the ozone-depleting reaction \(\mathrm{O}(g)+\mathrm{O}_{3}(g) \longrightarrow 2 \mathrm{O}_{2}(g)\) is \(7.9 \times 10^{-15} \mathrm{~cm}^{3} /\) molecule \(\cdot\) s. Express the rate constant in units of \(1 / M \cdot \mathrm{s}\)

Explain what is meant by the rate law of a reaction.

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 reaction $$ \mathrm{X}+\mathrm{Y} \longrightarrow \mathrm{Z} $$ From the following data, obtained at \(360 \mathrm{~K}\), (a) determine the order of the reaction, and (b) determine the initial rate of disappearance of \(\mathrm{X}\) when the concentration of \(\mathrm{X}\) is \(0.30 \mathrm{M}\) and that of Y is \(0.40 \mathrm{M}\). $$ \begin{array}{ccc} \hline \text { Initial Rate of } & & \\ \text { Disappearance of } \mathbf{X}(\boldsymbol{M} / \mathbf{s}) & {[\mathrm{X}](M)} & {[\mathrm{Y}](M)} \\ \hline 0.053 & 0.10 & 0.50 \\ 0.127 & 0.20 & 0.30 \\ 1.02 & 0.40 & 0.60 \\ 0.254 & 0.20 & 0.60 \\ 0.509 & 0.40 & 0.30 \\ \hline \end{array} $$

Cyclobutane decomposes to ethylene according to the equation $$ \mathrm{C}_{4} \mathrm{H}_{8}(g) \longrightarrow 2 \mathrm{C}_{2} \mathrm{H}_{4}(g) $$ Determine the order of the reaction and the rate constant based on the following pressures, which were recorded when the reaction was carried out at \(430^{\circ} \mathrm{C}\) in a constant-volume vessel. $$ \begin{array}{rc} \hline \text { Time (s) } & P_{\mathrm{C}_{4} \mathrm{H}_{8}}(\mathrm{mmHg}) \\\ \hline 0 & 400 \\ 2,000 & 316 \\ 4,000 & 248 \\ 6,000 & 196 \\ 8,000 & 155 \\ 10,000 & 122 \\ \hline \end{array} $$
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