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Chapter 14: Problem 57

Suggest experimental means by which the rates of the following reactions could be followed: (a) \(\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)\) (b) \(\mathrm{Cl}_{2}(g)+2 \mathrm{Br}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(a q)+2 \mathrm{Cl}^{-}(a q)\) (c) \(\mathrm{C}_{2} \mathrm{H}_{6}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2}(g)\)

Short Answer

Expert verified
The rate of reaction can be followed in accordance with the nature of the chemicals involved in every reaction. For reaction (a), the progress can be tracked by monitoring the production of \(CO_2\) gas, for reaction (b), by observing the change in the solution’s color characteristic of the Bromine product, and for reaction (c), by using a mass spectrometer to detect the production of \(H_2\) gas.

Step by step solution

01

Reaction (a) Approach

The reaction involves a solid (Calcium Carbonate: \(CaCO_3\)) converting to another solid (Calcium Oxide: \(CaO\)) and a gas (Carbon Dioxide: \(CO_2\)). The rate of this reaction can be monitored by observing the production of \(CO_2\) gas which can be measured using a mass spectrometer, otherwise, gas pressure can be monitored. This reaction can also be tracked visually if the reaction is set up in a closed system and a gas pressure sensor is attached to the system.
02

Reaction (b) Approach

In this reaction, a gaseous element (Chlorine: \(Cl_2\)) reacts with aqueous ions (Bromide ions: \(Br^-\)) to produce an aqueous compound (Bromine: \(Br_2\)) and another aqueous ion (Chloride ion: \(Cl^-\)). This reaction can be monitored by observing the change in color which is characteristic of the Bromine product, as it is a brown liquid. Additionally, electronic techniques could be used to track changes in ion concentration which would signal a reaction is occurring.
03

Reaction (c) Approach

The reaction involves a gas (Ethane: \(C_2H_6\)) converting to another gas (Ethene: \(C_2H_4\)) and Hydrogen gas (\(H_2\)). The most straightforward way of monitoring this reaction is to use a mass spectrometer to track the production of \(H_2\) gas. A gas pressure sensor could also be affixed to a closed system to track any pressure changes, which would signal a reaction.

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Most popular questions from this chapter

Write the reaction rate expressions for these reactions in terms of the disappearance of the reactants and the appearance of products: (a) \(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{HI}(g)\) (b) \(2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)\) (c) \(5 \mathrm{Br}^{-}(a q)+\mathrm{BrO}_{3}^{-}(a q)+6 \mathrm{H}^{+}(a q) \longrightarrow\) $$ 3 \mathrm{Br}_{2}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l) $$

The bromination of acetone is acid-catalyzed: \(\mathrm{CH}_{3} \mathrm{COCH}_{3}+\mathrm{Br}_{2} \frac{\mathrm{H}^{+}}{\text {catalyst }} \mathrm{CH}_{3} \mathrm{COCH}_{2} \mathrm{Br}+\mathrm{H}^{+}+\mathrm{Br}\) The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and \(\mathrm{H}^{+}\) ions at a certain temperature: $$ \begin{array}{lcllc} & & & & {\text { Rate of }} \\ & & & & \text { Disappearance } \\ & {\left[\mathrm{CH}_{3} \mathrm{COCH}_{3}\right]} & {\left[\mathrm{Br}_{2}\right]} & {\left[\mathrm{H}^{+}\right]} & \text {of } \mathrm{Br}_{2}(\mathrm{M} / \mathrm{s}) \\ \hline \text { (a) } & 0.30 & 0.050 & 0.050 & 5.7 \times 10^{-5} \\ \text {(b) } & 0.30 & 0.10 & 0.050 & 5.7 \times 10^{-5} \\ \text {(c) } & 0.30 & 0.050 & 0.10 & 1.2 \times 10^{-4} \\ \text {(d) } & 0.40 & 0.050 & 0.20 & 3.1 \times 10^{-4} \\ \text {(e) } & 0.40 & 0.050 & 0.050 & 7.6 \times 10^{-5} \end{array} $$ (a) What is the rate law for the reaction? (b) Determine the rate constant.

Define activation energy. What role does activation energy play in chemical kinetics?

What is meant by the rate of a chemical reaction?

When a mixture of methane and bromine is exposed to light, the following reaction occurs slowly: $$ \mathrm{CH}_{4}(g)+\mathrm{Br}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{Br}(g)+\mathrm{HBr}(g) $$ Suggest a reasonable mechanism for this reaction. (Hint: Bromine vapor is deep red; methane is colorless.)
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