Answer:
The rate equation for this reaction:
[tex]R=k[NH_3]^0[/tex]
Explanation:
Decomposition of ammonia:
[tex]2NH_3\rightarrow N_2+3H_2[/tex]
Rate law of the can be written as;
[tex]R=k[NH_3]^x[/tex]
1) Rate of the reaction , when [tex][NH_3]=2.0\times 10^{-3} M[/tex]
[tex]1.5\times 10^{-6} M/s=k[2.0\times 10^{-3} M]^x[/tex]..[1]
2) Rate of the reaction , when [tex][NH_3]=4.0\times 10^{-3} M[/tex]
[tex]1.5\times 10^{-6} M/s=k[4.0\times 10^{-3} M]^x[/tex]..[2]
[1] ÷ [2]
[tex]\frac{1.5\times 10^{-6}M/s}{1.5\times 10^{-6}M/s}=\frac{k[2.0\times 10^{-3}M]^x}{k[4.0\times 10^{-3}M]^x}[/tex]
On solving for x , we get ;
x = 0
The rate equation for this reaction:
[tex]R=k[NH_3]^0[/tex]
