Chlorine monoxide (ClO) decomposes at room temperature
according...

Question

Chlorine monoxide (ClO) decomposes at room temperature according to the reaction 2 ClO1g2¡Cl21g2 + O21g2 The concentration of ClO was monitored over time, and three graphs were made:

What is the rate law for the reaction? (LO 14.9) (a) Rate = k (b) Rate = k3ClO4 (c) Rate = k3ClO42 (d) Rate = k3ClO43 M14_MCMU6230_

Accepted Answer

Hello. In this problem we are told according to the reaction for the decomposition of nitrogen monoxide at 400 Celsius. Three graphs were created and the concentration of nitrogen monoxide was tracked throughout time. We are then asked what is the rate law for the decomposition reaction? So let's begin by looking at the three graphs. In this first graph we have concentration of nitrogen monoxide versus time. We call that a zero order reaction. Then the integrated rate law is given by the concentration of our reactant some time. T. Is equal to the negative of the reaction rate, constant times time plus the initial concentration about reacting. So if we make a plot of the concentration of nitric oxide versus time, if it is zero order, we should get a straight line or it should be linear. The we see that there's a bit of a curve, so it is not a zero order reaction. If we look at the next plot, we have the natural log of the concentration of nitrogen monoxide versus time. And if we recall a first order reaction then has an integrated rate law of the natural log of the concentration of our reactant is a function of time. Alright, sorry, time, T. Is equal to the negative of the reaction rate, constant times time plus the natural log of our reactant. Its initial concentration and a plot then of the natural log of concentration of nitric oxide versus time would give a linear fit, which this one appears to have and last one, we have one over concentration of nitric oxide versus time. The integrated rate law then, or a second order reaction recall is given by one over the concentration of our reactant at some time. T is equal to negative of the reaction rate constant times time plus one over the initial concentration of our reactant. So a plot of one over the concentration of nitric oxide versus time. If it gives a straight line, it would be second order, this is again curved, so it is not second order. We had a linear fit for a first order reaction, so the decomposition of nitrogen monoxide is first order. So if we look at the rate law, then the rate law for a first order reaction would be given by the rate is equal to the reaction rate, constant times the concentration of nitrogen monoxide to the first power. And so if we look at our answers that are provided, we find then that c. Is the correct answer. The rate then, is for a first order reaction. Thanks for watching Help. This helps

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