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How will each of the following affect the rate of the reaction: ${CO}(g)+{NO}_{2}(g) \rightarrow {CO}_{2}(g)+{NO}(g)$ if the rate law for the reaction is rate $=k[{NO}_{2}][{CO}] ?$(a) Increasing the pressure of ${NO}_{2}$ from 0.1 atm to 0.3 ${atm}$(b) Increasing the concentration of ${CO}$ from 0.02 ${M}$ to 0.06 ${M} .$
A. Hence, the rate of reaction triples when the pressure of $\mathrm{NO}_{2}$ increases from 0.1 atm to 0.3 atm.B. Therefore, the rate of reaction triples on increasing the concentration of $\mathrm{CO}$ increases from 0.02 $\mathrm{M}$ to $0.06 \mathrm{M} .$
Chemistry 102
Chapter 12
Kinetics
Carleton College
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Hello, everyone, this is Ricky. And today we're working on chapter 12 problem 16 and we have to calculate, but we have to determine how different changes will affect the rate of reaction. So first, if we increase the pressure and a two from 0.1 hmm. To white free, you too. All right. So we see that, um, in this case, the concentration of energy, too, is proportional two. Yeah. Pressure. Directly. And so we can substitute pressure Innertube in for concentration. Been up to, um, And so if we have a three fold increase in concentration of energy too, we'll have a three fold increase in reaction reeked. What is this? Um, reaction is first ordered turned in regards to, you know to now, if we the second change that we're making is increasing CEO concentration from point A to moller 2.6 Bowling. Now, this is an overall threefold increase in concentration. And what you'll see is that the rate of reaction will triple by increasing the concentration by three fold. And this has to do with facts that, um where first order in regard to carbon monoxide. So
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