The following reaction occurs in aqueous solution: NH4 + (aq) + NO2 - â†’ N2 (g) + 2H2O (l) The data below is obtained at 25Â°C. [NH4 +] (M) [NO2 -] (M) Initial rate (M/s) 0.0100 0.200 3.2 Ã— 10-3 0.0200 0.200 6.4 Ã— 10-3 The order of the reaction in NH4 + is __________.

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

[tex]NH_4^++NO_2^-\rightarrow N_2+2H_2O[/tex]

[tex]Rate=k[NH_4^+]^x[NO_2^-]^y[/tex]

k= rate constant

x = order with respect to [tex]NH_4^+[/tex]

y = order with respect to A[tex]NO_2^-[/tex]

n = x+y = Total order

From trial 1: [tex]3.2\times 10^{-3}=k[0.0100]^x[0.200]^y[/tex] (1)

From trial 2: [tex]6.4\times 10^{-3}=k[0.0200]^x[0.200]^y[/tex] (2)

Dividing 2 by 1 :[tex]\frac{6.4\times 10^{-3}}{3.2\times 10^{-3}}=\frac{k[0.0100]^x[0.2000]^y}{k[0.0200]^x[0.200]^y}[/tex]

[tex]2=2^x,2^1=2^x[/tex] therefore x= 1

Thus order with respect to [tex]NH_4^+[/tex] is 1.