Question

Consider the following reaction: 2NO(g)+2H2(g)→N2(g)+2H2O(g). The rate law for this reaction is first order in H2 and second order in NO. Write the rate law. The rate law for this reaction is first order in and second order in . Write the rate law. rate=k[H2][NO] rate=k[H2][NO]2 rate=k[H2]2[NO]2 rate=k[H2]

Answer 1

Answer:

k * [H2]*[NO]²

Explanation:

2NO(g) + 2H2 (g) → N2 (g) + 2H2O (g)

Rate law  = k*[A]^x *[B]^y

with k = rate constant

with [A] = concentration of A

with [B] = concentration of B

x and y are the orders of A and B respectively.

Rate is defined as: decrease in the concentration of reactants / time

For the given reaction:

⇒first order in H2 ⇔  rate α = [H2]∧1

⇒second order in NO ⇔ rate α = [NO]²

Rate law:

⇒then x =order of A = 1

⇒then y = order of B = 2

⇒Total order 1+2 =3 ⇒ third order