Question

6. The rate constant for the second-order reaction (shown below) is 0.54 M?¹s?¹ at 300°C. 2NO? (g) ? 2NO (g) + O? (g) What is the concentration of NO? after 7.4 s if the initial concentration of NO? is 0.65M?

          6. The rate constant for the second-order reaction (shown below) is 0.54 M?¹s?¹ at 300°C.
2NO? (g) ? 2NO (g) + O? (g)
What is the concentration of NO? after 7.4 s if the initial concentration of NO? is 0.65M?

Added by Brent V.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Adi S

06/27/2022

Step 1

Step 1: Write down the rate law for the given second-order reaction: The rate law for a second-order reaction is given by: rate = k[NO2]^2 where: rate = rate of reaction k = rate constant [NO2] = concentration of NO2 Show more…

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The rate constant for the second-order reaction (shown below) is 0.54M^(-1)s^(-1) at 300deg C. 2NO_(2(g))longrightarrow2NO_((g))+O_(2(g)) What is the concentration of NO_(2) after 7.4s if the initial concentration of NO_(2) is 0.65M ? What is the concentration of NOz after 7.4 s if the initial concentration of NOz is 0.65M? 6.The rate constant for the second-order reaction (shown below) is 0.54 M-1s-1 at 300C.