Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) The rate law

Question

Consider the following reaction:

2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)


The rate law for this reaction is second order in NO(g) and first order in H2(g). Pick the correct rate law for this reaction from the multiple choices.


The answer below is E but my question is how do you determine the Rate Law? I'm so confused about what to specifically look for or pay attention to in the reaction above. Please have Details. I will rate!! :)

a) Rate = k [NO(g)] [H2(g)]
b) Rate = k [NO(g)]4 [H2(g)]
c) Rate = k [NO(g)] [H2(g)]2
d) Rate = k [NO(g)] [H2(g)]4
e) Rate = k [NO(g)]2 [H2(g)]

Explanation / Answer

e) Rate = k [NO(g)]2 [H2(g)] If Rate is of x order in Y, then Rate is proportional to [Y]^x =>Rate = k1*[Y]^x Similarly if Rate is of u order in V, then Rate is proportional to [V]^u =>Rate = k2*[V]^u Now multiply both rates to get Rate = k1k2[Y]^x[V]^u where k1 and k2 are constants. Let k = k1k2 =>Rate = k[Y]^x[V]^u

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.