1) Substance A and B react to form B and C by the following reaction. The initia

Question

1) Substance A and B react to form B and C by the following reaction. The initial rate of reaction is 2.0 M/s. What is the initial rate of change of A, B, C and D?

A+3B?2C+3D

2) Nitrogen dioxide has an initial concentration of 6.0 M. At 2, 4 and 8 hours the concentration is 4.0 M, 2.0 M and zero. What is the average rate of reaction in the first two hours (in M/hr)? What is the average rate over the last four hours? What is the instantaneous rate at 9 hours?

2N2O?2N2 +O2

3) If the following reaction is first order what differential rate law would describe the reaction rate? If it is a second order reaction, what would be the differential rate law?

2H2O2 ?2H2O+O2

4) The rate constant (k) for a zero order reaction is 3.981x10-2. What is the reaction rate? (hint: the differential rate laws relate concentration to rate of reaction)

5) A first order reaction is 45.0% complete in 65 s. What is the rate constant (k) in s-1? (hint: the integrated rate law relates concentration to time)

Explanation / Answer

Ans 1

The given reaction is

A + 3B = 2C + 3D

Relation between rate of reaction of reactants and products

rA/(-1) = rB/(-3) = rC/(2) = rD/(3)

initial rate of reaction = 2.0 M/s

rA = - 2 M/s

rA/(-1) = rB/(-3)

rB = 3 rA = 3 x (-2 M/s) = - 6 M/s

rC = - 2 x rA = - 2 x (-2 M/s) = 4 M/s

rD = - 3 x rA = - 3 x (-2 M/s) = 6 M/s

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