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Chapter 13: Problem 41

\(\Delta\) (Any quantity) is always defined as (final value of quantity) - (initial value of quantity). Now consider the quantity \(\Delta E_{\mathrm{rxn}}\). (a) For the forward reaction \(\mathrm{R} \rightarrow \mathrm{P}\), is \(\Delta E_{\mathrm{rxn}}=E_{\text {Reactants }}-E_{\text {Products }} ?\) Explain your answer. (b) According to your answer to (a), what does it mean when \(\Delta E_{\mathrm{rxn}}\) for a reaction is negative?

Short Answer

Expert verified
(a) Yes, for the forward reaction \(R \rightarrow P\), \(\Delta E_{\mathrm{rxn}} = E_{\text{Products}} - E_{\text {Reactants}}\), as it represents the difference in energy between the final state (products) and the initial state (reactants). (b) When \(\Delta E_{\mathrm{rxn}}\) is negative, it means the energy of the products is lower than the energy of the reactants. This indicates that the reaction is exothermic, as energy is released to the surroundings during the reaction.

Step by step solution

01

(Part (a): Analyzing the definition of ΔErxn)

(The given definition of Δ (Any quantity) is "final value of quantity - initial value of quantity." In a chemical reaction, the final state is when products are formed, and the initial state is when reactants were present before the reaction took place. Hence, for the forward reaction \(\mathrm{R} \rightarrow \mathrm{P}\), \(\Delta E_{\mathrm{rxn}}\) can be defined as: \[\Delta E_{\mathrm{rxn}} = E_{\text{Products}} - E_{\text {Reactants}}\])
02

(Part (a): Explanation)

(According to the definition we derived above, the value of \(\Delta E_{\mathrm{rxn}}\) is equal to the difference between energies of products and reactants, which confirms that: \(\Delta E_{\mathrm{rxn}} = E_{\text {Products }} - E_{\text {Reactants }}\)
03

(Part (b): Significance of negative ΔErxn)

(When \(\Delta E_{\mathrm{rxn}}\) is negative, it means the energy of the products is lower than the energy of the reactants: \(\Delta E_{\mathrm{rxn}}<0 \Rightarrow E_{\text {Products }} < E_{\text {Reactants }}\) This implies that the reaction releases energy to the surroundings since the products have lower energy than the reactants, which indicates that the reaction is exothermic.)

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Most popular questions from this chapter

Regarding a chemical reaction's mechanism: (a) Suppose we could see individual molecules as they undergo a chemical reaction. Why might it still be difficult to directly observe the reaction's mechanism? (b) What do chemist typically do to indirectly "see" a reaction mechanism?

The mechanism for the reaction of \(A_{2}\) with \(B\) is: Step \(1: \mathrm{A}_{2}+\mathrm{Y} \rightarrow \mathrm{AY}+\mathrm{A}\) (slow) Step \(2: \mathrm{A}+\mathrm{B} \rightarrow \mathrm{AB}\) (fast) Step 3: \(\mathrm{AY}+\mathrm{AB} \rightarrow \mathrm{Y}+\mathrm{A}_{2} \mathrm{~B}\) (fast) (a) Write the overall reaction that is occurring. (b) Which step determines the rate law for the reaction? (c) Write the rate law for the reaction. (d) What happens to the rate of the reaction when \(\left[\mathrm{A}_{2}\right]\) is doubled? (e) Which species is the catalyst? (f) Which species are reaction intermediates?

Consider the transition state for a chemical reaction. (a) What is it (define it). (b) Can there be only imminent bond breaking in a transition state? Explain.

When a chemical reaction is in the ______________, the reactant bonds are just ready to break and the product bonds are just ready to form.

The reaction of Problem \(13.40\) is run in the reverse direction \((\mathrm{P} \rightarrow \mathrm{R})\). (a) Is it exothermic or endothermic? (b) Calculate \(\Delta E_{\mathrm{rxn}} .\) (c) Is what you just said and calculated for (a) and (b) consistent with the definition of \(\Delta\) (any quantity) given in Problem \(13.41\) ? Explain.
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