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Chapter 13: Problem 17

Write a general rate law for the reaction $$2 \mathrm{NO}+\mathrm{O}_{2} \rightarrow 2 \mathrm{NO}_{2}$$ using \(x\) and \(y\) as orders.

Short Answer

Expert verified
The general rate law for the reaction \(2 \mathrm{NO}+\mathrm{O}_{2} \rightarrow 2 \mathrm{NO}_{2}\) using \(x\) and \(y\) as orders is: \[\text{Rate} = k [\text{NO}]^x [\text{O}_{2}]^y \]

Step by step solution

01

Identify the reactants and their orders

In the reaction, the reactants are NO and O₂. The orders of the reactants are represented by x and y, respectively.
02

Write the general rate law

Using the general form of the rate law, substitute the reactants and their orders into the equation: Rate = k [NO]^x [O₂]^y where Rate is the reaction rate, k is the rate constant, [NO] and [O₂] are the concentrations of NO and O₂, and x and y are their respective orders. So, the general rate law for the given reaction is: \[\text{Rate} = k [\text{NO}]^x [\text{O}_{2}]^y \]

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Most popular questions from this chapter

A student says to you, "Catalysts are not used up in chemical reactions because they are not involved in the reactions." Is this statement true or false? Why?

Which branch of chemistry concerns itself with the study of reaction rates and the factors that affect rates?

A student claims that an endothermic reaction will always have a higher activation energy than an exothermic reaction, because an endothermic reaction ends up with the products at a higher energy than the reactants. Is this correct or incorrect? Justify your answer.

For a particular chemical reaction, the absorbed energy is \(800 \mathrm{~kJ}\) to break old bonds, and \(400 \mathrm{~kJ}\) is released on forming new bonds. Calculate \(\Delta E_{\mathrm{rxn}}\) and comment on whether this reaction is exothermic or endothermic. Explain why.

Indicate whether each statement is true or false. Rewrite each false statement to make it true. (a) The exponents in the rate law for a reaction that has a one-step mechanism can be determined from the balanced equation for the reaction. (b) A rate law can be used to prove that a proposed mechanism is correct. (c) The step \(\mathrm{A}+\mathrm{X}+\mathrm{Y} \rightarrow \mathrm{AX}+\mathrm{Y}\) in a reaction mechanism is plausible. (d) A reaction intermediate appears first as a reactant and then as a product in a reaction mechanism.
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