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Chapter 13: Problem 9

Consider the reaction \(\mathrm{A}_{2}+\mathrm{B}_{2} \rightarrow 2 \mathrm{AB}\), for which \(\Delta E_{\mathrm{rxn}}=-100 \mathrm{~kJ}\). Forming 1 mole of A \(-B\) bonds releases \(150 \mathrm{~kJ}\). How much energy does it take to break the reactant bonds?

Short Answer

Expert verified
It takes 200 kJ of energy to break the reactant bonds in the reaction \(A_{2}+B_{2} \rightarrow 2AB\), where \(\Delta E_{rxn} = -100 \text{kJ}\) and forming 1 mole of AB bonds releases 150 kJ of energy.

Step by step solution

01

Identify the given information

We are given: - ΔErxn = -100 kJ - Energy released to form 1 mole of AB bonds = 150 kJ
02

Write the energy balance equation

Using the given information, write the energy balance equation for this reaction: ΔErxn = Energy required to break reactant bonds - Energy released to form product bonds
03

Calculate the energy released to form product bonds

Since 1 mole of A2 and B2 yields to 2 moles of AB, we need to multiply the energy released to form 1 mole of AB bonds by 2 to find the energy released to form 2 moles of AB bonds: Energy released to form 2 moles of AB bonds = 150 kJ/mol × 2 = 300 kJ
04

Calculate the energy required to break reactant bonds

Now, substitute the values of ΔErxn and the energy released to form product bonds into the energy balance equation: -100 kJ = Energy required to break reactant bonds - 300 kJ To find the energy required to break reactant bonds, add 300 kJ to both sides of the equation: Energy required to break reactant bonds = -100 kJ + 300 kJ = 200 kJ So, it takes 200 kJ of energy to break the reactant bonds.

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Most popular questions from this chapter

Ace chemistry student Sidney Einstein (no relation) was carrying out a kinetics experiment in lab which produces iodine and uses starch as an indicator. In the first minute after mixing, Sidney spilled some of the solution. Rather than start over, he decided to pour out more solution until he had exactly half the original volume in the tube. Given that the particular reaction under investigation was second order in the reactant being investigated and was supposed to change color after 10 minutes, approximately how long (minutes) will it be before Sidney sees a color change? Explain briefly!

Which of the following are substitution reactions: (a) \(\mathrm{CH}_{3} \mathrm{Br}+\mathrm{I}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{I}+\mathrm{Br}^{-}\) (b) \(\mathrm{H}_{2}+\mathrm{Br}_{2} \rightarrow 2 \mathrm{HBr}\) (c) \(\mathrm{CH}_{2}=\mathrm{CH}_{2}+\mathrm{H}_{2} \rightarrow \mathrm{CH}_{3}-\mathrm{CH}_{3}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Cl}+\mathrm{OH}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{Cl}^{-}\)

Given the rate data below from a series of kinetics experiments, determine the orders for the following reaction, and state the overall order of the reaction: \(\mathrm{H}_{2} \mathrm{O}_{2}(a q)+3 \mathrm{I}^{-}(a q)+2 \mathrm{H}^{+}(a q) \rightarrow \mathrm{I}_{3}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\) $$\begin{array}{cccc} \text { Experiment }\left[\mathbf{H}_{2} \mathrm{O}_{2}\right] & {\left[\mathbf{I}^{-}\right]} & {\left[\mathbf{H}^{+}\right]} & \text {Rate }(\mathbf{M} / \mathbf{s}) \\ \hline 1 & 0.010 \mathrm{M} & 0.010 \mathrm{M} & 0.00050 \mathrm{M} & 1.15 \times 10^{-6} \\ 2 & 0.020 \mathrm{M} & 0.010 \mathrm{M} & 0.00050 \mathrm{M} & 2.30 \times 10^{-6} \\ 3 & 0.010 \mathrm{M} & 0.020 \mathrm{M} & 0.00050 \mathrm{M} & 2.30 \times 10^{-6} \\ 4 & 0.010 \mathrm{M} & 0.010 \mathrm{M} & 0.00100 \mathrm{M} & 1.15 \times 10^{-6} \end{array}$$

In a chemical reaction, compound A is converted to compound \(\mathrm{B}\). In the process, energy is absorbed from the surroundings. Which compound is at a higher energy level? Explain your answer.

Suppose you increase the temperature of a reaction from \(100^{\circ} \mathrm{C}\) to \(200^{\circ} \mathrm{C}\) and the reaction gets three times as fast. (a) Would the rate constant for the reaction at \(100^{\circ} \mathrm{C}\) be equal to the rate constant for the reaction at \(200^{\circ} \mathrm{C}\) ? (b) Suppose you took a ratio \(k_{200^{\circ} \mathrm{C}} / k_{100^{\circ} \mathrm{C}}\). According to the information given in part (a), what would you expect the value of this ratio to be?
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