Question

Please use the values in the resources listed below instead of the textbook values. Under certain conditions the decomposition of ammonia on a metal surface gives the following data.[NH3] (M) 2.0 ✕ 10−3 4.0 ✕ 10−3 6.0 ✕ 10−3 Rate (mol/L/h) 1.5 ✕ 10−6 1.5 ✕ 10−6 1.5 ✕ 10−6 Determine the rate equation for this reaction. (Rate expressions take the general form: rate = k . [A]a . [B]b.)

Answer 1

Answer:

The rate equation for this reaction:

$R=k[NH_3]^0$

Explanation:

Decomposition of ammonia:

$2NH_3\rightarrow N_2+3H_2$

Rate law of the can be written as;

$R=k[NH_3]^x$

1) Rate of the reaction , when $[NH_3]=2.0\times 10^{-3} M$

$1.5\times 10^{-6} M/s=k[2.0\times 10^{-3} M]^x$..[1]

2) Rate of the reaction , when $[NH_3]=4.0\times 10^{-3} M$

$1.5\times 10^{-6} M/s=k[4.0\times 10^{-3} M]^x$..[2]

[1] ÷ [2]

$\frac{1.5\times 10^{-6}M/s}{1.5\times 10^{-6}M/s}=\frac{k[2.0\times 10^{-3}M]^x}{k[4.0\times 10^{-3}M]^x}$

On solving for x , we get ;

x = 0

The rate equation for this reaction:

$R=k[NH_3]^0$