Rate Law concentration problem...giving me trouble. Help?

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For the reaction, A(g) + B(g) => AB(g), the rate is 0.270 mol/L.s when the initial concentrations of both A and B are 2.00 mol/L. If the reaction is second order in A and second order in B, what is the rate when the initial concentration of A = 3.93 mol/L and that of B = 1.92 mol/L. I get 3.84 but the correct response is .96
 
Well the problem is that your rate constant's units imply an overall reaction order of 2. And if your reaction is elementary, then the reactions should be 1st order in A and 1st order in B. your rate law should read:

r=-k[A]
 
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