For a reaction, 2NO + 2H2 → N2 + 2H2O, the possible mechanism is 2NO leftharpoons N2O2 N2O2+H2 xrightarrow textslow N2O+H2O N2O+H2O xrightarrow textfast N2+H2O What is the rate law and order of the reaction?

Question

For a reaction, 2NO + 2H2 → N2 + 2H2O, the possible mechanism is 2NO leftharpoons N2O2 N2O2+H2 xrightarrow textslow N2O+H2O N2O+H2O xrightarrow textfast N2+H2O What is the rate law and order of the reaction? (A) Rate = [N2O2], order = 1 (B) Rate = [N2O2] [H2], order = 2 (C) Rate = [N2O2]2, order = 2 (D) Rate = [N2O2]2 [H2], order = 3

Tardigrade Admin · Accepted Answer

The slowest step of the reaction is rate determining step N2O2+ H2 → N2O+ H2O Rate of reaction = [N2O2] [H2] Hence, order of reaction = 2

Q. For a reaction, $2 NO + 2 H_{2} \to N_{2} + 2 H_{2} O$ , the possible mechanism is
$2 NO ⇌ N_{2} O_{2}$
$N_{2} O_{2} + H_{2} slow N_{2} O + H_{2} O$
$N_{2} O + H_{2} O fast N_{2} + H_{2} O$
What is the rate law and order of the reaction?

Rate $= [N_{2} O_{2}]$ , order $= 1$

Rate $= [N_{2} O_{2}] [H_{2}]$ , order $= 2$

Rate $= [N_{2} O_{2}]^{2}$ , order $= 2$

Rate $= [N_{2} O_{2}]^{2} [H_{2}]$ , order $= 3$

The slowest step of the reaction is rate determining step
$N_{2} O_{2} + H_{2} \to N_{2} O + H_{2} O$
Rate of reaction $= [N_{2} O_{2}] [H_{2}]$
Hence, order of reaction $= 2$

Q. For a reaction, 2NO+2H2​→N2​+2H2​O, the possible mechanism is 2NO⇌N2​O2​ N2​O2​+H2​slow​N2​O+H2​O N2​O+H2​Ofast​N2​+H2​O What is the rate law and order of the reaction?

Rate =[N2​O2​], order =1

Rate =[N2​O2​][H2​], order =2

Rate =[N2​O2​]2, order =2

Rate =[N2​O2​]2[H2​], order =3