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Chapter 1: Problem 6

Which of the following is true for an endothermic reaction? (A) The strength of the bonds in the products exceeds the strength of the bonds in the reactants. (B) The activation energy is always greater than the activation energy for an exothermic reaction. (C) Energy is released over the course of the reaction. (D) A catalyst will increase the rate of the reaction by increasing the activation energy.

Short Answer

Expert verified
After evaluating all the options, it can be concluded that none of the options (A, B, C, or D) provided are true for an endothermic reaction.

Step by step solution

01

Understanding Endothermic Reactions

Endothermic reactions are those where energy (in the form of heat) is absorbed from the surroundings. This type of reaction often feels cold, because it's taking heat away from what it's reacting with - like a hot sidewalk or your skin.
02

Analyzing Option A

Option A is incorrect. The strength of the bonds in the products exceeding the strength of the bonds in the reactants is independent of the reaction being endothermic or exothermic. This has more to do with the specific chemical properties of the reactants and products rather than the type of reaction.
03

Analyzing Option B

Option B is also incorrect. The activation energy has no direct correlation with whether a reaction is endothermic or exothermic. Both types of reactions require an initial amount of energy to start and this 'activation energy' can be different for each reaction, regardless of the type of reaction.
04

Analyzing Option C

Option C is incorrect. An endothermic reaction is characterized by the absorption of heat, not its release. This is the reverse of what is stated in option C. Thus, this statement is false.
05

Analyzing Option D

Option D is incorrect. A catalyst does increase the rate of reaction, but this is by lowering the activation energy, not increasing it.

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Most popular questions from this chapter

A laboratory technician wishes to create a buffered solution with a pH of 5. Which of the following acids would be the best choice for the buffer? (A) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \quad K_{a}=5.9 \times 10^{-2}\) (B) \(\mathrm{H}_{3} \mathrm{AsO}_{4} \quad K_{a}=5.6 \times 10^{-3}\) (C) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \quad K_{a}=1.8 \times 10^{-5}\) (D) \(\mathrm{HOCl}\) \(\quad K_{a}=3.0 \times 10^{-8}\)

Use the following information to answer questions 29-31. Pennies are made primarily of zinc, which is coated with a thin layer of copper through electroplating, using a setup like the one above. The solution in the beaker is a strong acid (which produces H' ions), and the cell is wired so that the copper electrode is the anode and zinc penny is the cathode. Use the following reduction potentials to answer questions \(29-31 .\) $$\begin{array}{|l|l|}\hline \text { Half-Reaction } & {\text { Standard Reduction Potential }} \\ \hline \mathrm{Cu}^{2++2 e^{-} \rightarrow \mathrm{Cu}(s)} & {+0.34 \mathrm{V}} \\ \hline 2 \mathrm{H}^{++2 e^{-} \rightarrow \mathrm{H}_{2}(g)} & {0.00 \mathrm{V}} \\ \hline \mathrm{Ni}^{2++2 e^{-} \rightarrow \mathrm{Ni}(s)} & {-0.25 \mathrm{V}} \\\ \hline \mathrm{Zn}^{2++2 e^{-} \rightarrow \mathrm{Zn}(s)} & {-0.76 \mathrm{V}} \\ \hline\end{array}$$ What is the required voltage to make this cell function? (A) 0.34 V (B) 0.42 V (C) 0.76 V (D) 1.10 V

Use the following information to answer questions 1-5. \(\begin{array}{ll}{\text { Reaction } 1 : \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2}(g) \rightarrow 2 \mathrm{NH}_{3}(g)} & {\Delta H=?} \\ {\text { Reaction } 2 : \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{CH}_{4} \mathrm{O}(l) \rightarrow \mathrm{CH}_{2} \mathrm{O}(g)+\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g)} & {\Delta H=-37 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}} \\ {\text { Reaction } 3 : \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightarrow 2 \mathrm{NH}_{3}(g)} & {\Delta H=-46 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}} \\ {\text { Reaction } 4 : \mathrm{CH}_{4} \mathrm{O}(l) \rightarrow \mathrm{CH}_{2} \mathrm{O}(g)+\mathrm{H}_{2}(g)} & {\Delta H=-65 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}}\end{array}\) What is the enthalpy change for reaction 1\(?\) (A) \(-148 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (B) \(-56 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (C) \(-18 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (D) \(+148 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\)

Molten \(\mathrm{AlCl}_{3}\) is electrolyzed with a constant current of 5.00 amperes over a period of 600.0 seconds. Which of the following expressions is equal to the maximum mass of Al(s) that plates out? (1 faraday = 96,500 coulombs) (A) \(\frac{(600)(5.00)}{(96,500)(3)(27.0)}\) grams (B) \(\frac{(600)(5.00)(3)(27.0)}{(96,500)}\) grams (C) \(\frac{(600)(5.00)(27.0)}{(96,500)(3)}\) grams (D) \(\frac{(96,500)(3)(27.0)}{(600)(5.00)}\) grams

A proposed mechanism for a reaction is as follows: $\begin{array}{cc}{\mathrm{NO}_{2}+\mathrm{F}_{2} \rightarrow \mathrm{NO}_{2} \mathrm{F}+\mathrm{F}} & {\text { Slow step }} \\ {\mathrm{F}+\mathrm{NO}_{2} \rightarrow \mathrm{NO}_{2} \mathrm{F}} & {\text { Fast step }}\end{array}$ What is the order of the overall reaction? (A) Zero order (B) First order (C) Second order (D) Third order
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