10, 11, and 12 please show how you came to that answer 10. A general reaction wr

Question

10, 11, and 12
please show how you came to that answer

10. A general reaction written as 2A + 2B C + 2D i studied and yields the tallowing data Initial Initial [A 0.100 0.100 0.200 0,000040 Ms 0.000160 Ms 0.000040 Ms 7 0.200 0.100 Vhat is the order of the reaction with respect to B? 2 B1 COD For the reaction described in problem 10, what is the order of the reaction with respect to A? C. 0 D. 1 11. E. 2 12. NO reacts with chlorine in a gas phase reaction to form nitrosyl chloride, NOC1. From the following experimental data, determine the form of the equation that describes the relationship of reaction rate to initial concentrations of reactants. 2NO + Cl 2NOCI Initial Rate of Formation of NOCI 1.14 M/hr 9.12 Mhr 4.56 M/hr Initial INO) 0.50 1.00 1.00 0.50 1.00 0.50 A. Rate-k[NO] C. Rate =k[NO]2 E. Rate = k[NO]2[Cl2r B, Rate k[NOTC] D. Rate-k(NOFIC]

Explanation / Answer

10. C) 0

The reaction is zero order with respect to B.

From experiments 1 and 3:

[A]1 = [A]3 = 0.100 M

[B]1 = 0.100 M,        [B]3 = 0.200 M

R1 = R3 = 0.000040 M/s

Keeping the concentration of A constant, when concentration of B is doubled, the rate of the reaction does not change. Hence, the rate is independent of concentration of B. So, it is zero order with respect to B.

11. E)2

The reaction is second order with respect to A.

From experiments 1 and 2:

[A]1 = 0.100 M         [A]3 = 0.200 M

[B]1 = [B]3 = 0.100 M      

R1 = 0.000040 M/s       R3 = 0.000160 M/s = 4 R1

keeping concentration of B constant, on doubling the concentration of A, the rate becomes 4 times. So, rate of reaction must be second order with respect to A.

Rate = k[A]2[B]0

when R is proportional to [A]2, on doubling A, rate becomes [2A]2 = 4A2. So, rate becomes 4 times.

12. D) Rate = k[NO]2[Cl2]

From experiments 1 and 3: keeping concentration of [Cl2] constant, when [NO] is doubled, rate beomes 4 times. Hence, the reaction is second order with respect to NO.

From experiments 2 and 3: keeping concentration of [NO] constant, when [Cl2] is halved, rate is halved. Hence, the reaction is first order with respect to Cl2.

Hence the rate of the reaction is

Rate = k[NO]2[Cl2]

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