Given the initial rate data for the reaction A + B at 25 degree C, the rate law

Question

Given the initial rate data for the reaction A + B at 25 degree C, the rate law expression is given by k [A]a [B]b (a)Determine the reaction orders a and b. (b) (2 pt) if the reaction temperature become 10^0C, Which of the following statements is correct? Explain your choice (one or more than one answers) (1) The reaction rate for the trial consisting of [A]= 0.0344M and [B] = 0.160 M will increase -(ii) The reaction rate for the trial consisting of [A] = 0.0516M and [B] = 0.160 M will increase (iii) The reaction rate for the trial consisting of [A] = 0.0516M and [B] = 0.160 M will not change (iv) The reaction rate for the trial consisting of [A] = 0.0516M and [B] = 0.160 M will decrease (v) None of above

Explanation / Answer

a) let's do first part

now look at the dta given

we see than in 1st and 2nd data concentration of A is same while concentration on B increased 1.5 times (0.516/0.344 =1.5)

concentration of C also increases 1.5 times (3.17/2.11 =1.5)

so b=1

now look and 1st and 3rd data

concentration of A increases 1.7 times then concentration of C increases 2.89 (1.7*1.7) times

so a=2

rate law = k [A]2 [B]

b) order of reaction is 3

since k increases with decrease in temperature

so as temperature decreases rate increases

So a and b are correct options

Related Questions

Navigate

• Browse (All)
• Browse G
• Subjects

---

---

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