Asked by Anonymous
Ammonium ion (NH4^+) reacts with nitrite ion (NO2^-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations.
Expt. # [NH4^+] [NO2^-] Initial rate (M/hr)
1 0.010 0.020 0.020
2 0.015 0.020 0.030
3 0.030 0.010 0.015
What is the rate law (rate equation) for this reaction?
Answers
                    Answered by
            DrBob222
            
    How much of this can you do on your own. For example, have you determined that (NH4^+) is first order? (It is.)
For order of NO2^-
rate = k(NH4^+)(NO2^-)
rate2 = k(0.015)^1(0.020)^x
rate3 = k(0.030)^1(0.010)^x
Divide rate2 equation by rate3 eqn and solve for x. I obtained x = 2.
    
For order of NO2^-
rate = k(NH4^+)(NO2^-)
rate2 = k(0.015)^1(0.020)^x
rate3 = k(0.030)^1(0.010)^x
Divide rate2 equation by rate3 eqn and solve for x. I obtained x = 2.
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