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Rate Law and rate constant

IrishKnight · 2008-03-30 17:51:25

Given the below reaction 2NO+2H2 ---> N2+2H2O and the following data, how can I work out the rate law and the rate constant. [NO]/mol/L [H2]/mol/L Rate/mol/L/s 0.025 0.025 0.99x10^-4 0.050 0.025 3.96x10^-4 0.050 0.075 11.88x10^-4 I know that the rate=k[NO]^n[H2]^m But how do you work out n and m?

30-03-2008 05:51PM

#1

IrishKnight

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Posts: 842

Given the below reaction

2NO+2H2 ---> N2+2H2O

and the following data, how can I work out the rate law and the rate constant.

[NO]/mol/L [H2]/mol/L Rate/mol/L/s
0.025 0.025 0.99x10^-4
0.050 0.025 3.96x10^-4
0.050 0.075 11.88x10^-4

I know that the rate=k[NO]^n[H2]^m

But how do you work out n and m?

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Comments

#2 30-03-2008 06:12PM

Thomas_S_Hunterson

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Posts: 5948

AFAIK, n and m are the coefficients in the chamical equation, so 2 and 2 respectively.

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