Nitrogen monoxide, NO, reacts with hydrogen, H 2, according to the following equation: 2NO(g) + 2H2(g) arrow N2(g) + 2H2O(g) If the mechanism for this reaction were, 2 NO ( g )+ H 2( g ) arrow N 2( g )+ H 2 O 2( g ) ; text slow H 2 O 2( g )+ H 2( g ) arrow 2 H 2 O ( g ) ; text fast Which of the following rate laws would we expect to obtain experimentally?

Question

Nitrogen monoxide, NO, reacts with hydrogen, H 2, according to the following equation: 2NO(g) + 2H2(g) arrow N2(g) + 2H2O(g) If the mechanism for this reaction were, 2 NO ( g )+ H 2( g ) arrow N 2( g )+ H 2 O 2( g ) ; text slow H 2 O 2( g )+ H 2( g ) arrow 2 H 2 O ( g ) ; text fast Which of the following rate laws would we expect to obtain experimentally? (A) Rate =k[ H 2 O 2][ H 2] (B) Rate =k[ NO 2[ H 2]. (C) Rate =k[ NO 2[ H 2]2. (D) Rate =k[ NO ][ H 2]

Tardigrade Admin · Accepted Answer

Slow reaction is the rate determining step.

Rate $= k [H_{2} O_{2}] [H_{2}]$

Rate $= k [N O^{2} [H_{2}]$

Rate $= k [N O^{2} [H_{2}]^{2}$

Rate $= k [NO] [H_{2}]$

Slow reaction is the rate determining step.

Rate =k[H2​O2​][H2​]

Rate =k[NO2[H2​]

Rate =k[NO2[H2​]2

Rate =k[NO][H2​]

Slow reaction is the rate determining step.

Rate $= k [H_{2} O_{2}] [H_{2}]$

Rate $= k [N O^{2} [H_{2}]$

Rate $= k [N O^{2} [H_{2}]^{2}$

Rate $= k [NO] [H_{2}]$