Consider the initial-rate data at a certain temperature in...

Consider the initial-rate data at a certain temperature in the table for the reaction described by 2NO$_2$(g) + O$_3$(g) ? N$_2$O$_5$(g) + O$_2$(g) Determine the value and units of the rate constant, $k$. k = [NO$_2$]$_0$ (M) [O$_3$]$_0$ (M) Initial rate (M/s) 0.650 0.800 2.73 x 10$^{-4}$ 1.10 0.800 4.62 x 10$^{-4}$ 1.76 1.40 12.94 x 10$^{-4}$ Units:

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00:01 Hi, hello, see here they are asking to calculate the so the value of rate constant k value so they're asking to calculate so they given the reaction actually so the reaction they given that 2 and o2 2 no2 it's a gases molecule and reacting with o3 gases molecule so it forms n2 05 and o2 so for this they mentioned the values so actually for this reaction the rate will become what rate constant k multiplies with concentration of n o2 to the power a and concentration of o 3 so to the power b so this is the concentration terms so here they give it two experiments actually so here they mention the experiments three experiments they given so and so these n2 o2 values they mentioned and o3 values also they mentioned o3 concentration values and initial rates and initial rate also they mentioned so see in first so they mentioned that 0 .650 and 0 point so 800 and here 2 point so 2 1 multiplies with 10 to the power 4 second experiment they mentioned that 1 .1 so next experiment 0 .8 -00.

01:44 So here the initial rate they mentioned that 3 .74 multiplies with 10 to the power 4.

01:50 And experiment 3, 1 .76, 1 .40, 10 .47, multiplies with 10 to the power 4.

02:04 So they mentioned these.

02:05 So if you write the rate for all these three experiments, for suppose c, i am mentioning that one here.

02:14 For suppose, see, for experiment 1, if i mentioned the rate value, r1, will become that k multiplies with the concentration of no2, so concentration of o3.

02:30 So this is what they given to point, so 21 multiplies with 10 to the power 4.

02:35 So then this will become what actually, so r1 equal to, so k multiplies 0 .650...

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