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90% dow Help e teaching and i x CovalentActivity.do?locator-assignment-take&takeAssignmentSessionLocator-assig; Updates Ready to Some apps current preventing automat ? Use the References to access Impertant values If needed for this question. The decomposition of nitrous oxide at 565 °C N20(g)--N2(g) + ½ O2(g) is second order in N2O with a rate constant of 1.10x103M1s1 If the initial concentration of N20 is 0.755 M, the concentration of N20 will be M after 2.89x10 seconds have passed. Submit Answer Retry Entire Group 8 more group attempts remaining Next

Explanation / Answer

[N2O]t = 0.222 M

In a second order reaction, Rate = k[A]2, Integrated rate equation is given by the formula

1/[A]t - 1/[A]o = kt

[N2O]o = 0.755 M

k = 1.10 x 10-3 M-1 s-1

t = 2.89 x 103 s

i.e.   1/[N2O]t - 1/[N2O]o = kt

1/[N2O]t - 1/0.755 M = (1.10 x 10-3 M-1 s-1) x (2.89 x 103 s)

1/[N2O]t = 3.179 M-1 + 1/0.755 M =   3.179 M-1 + 1.3245 M-1 = 4.504 M-1

[N2O]t = 1/4.504 M-1 = 0.222 M

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