For Problems 3 through 6, consider the following reaction: 2 A + 4 B -> C + 4 D

Question

For Problems 3 through 6, consider the following reaction:

2 A + 4 B -> C + 4 D

The rate law for this reaction was experimen-
tally determined to be rate = k[A]2[B]3

PROBLEM 3:

What is the reaction order with respect to A?
1. 3/2
2. 3
3. 5
4. 2/3
5. 6
6. 2
7. 1

PROBLEM 4:

What is the reaction order with respect to B?
1. 3/2
2. 5
3. 3
4. 6
5. 1
6. 2
7. 2/3

PROBLEM 5:

If the initial concentration of A is increased
by a factor of 10 and the initial concentration
of B is simultaneously decreased by a factor
of 5, how will this affect the initial reaction
rate?
1. The rate would be one sixth of what it
was.
2. The rate would be four thirds of what it
was.
3. None of these answers are correct.
4. The rate would be unchanged.
5. The new rate would be 1.5 times faster
than before.
6. The rate would be doubled.
7. The new rate would be 2.5 times faster
than before.
8. The rate would be four fifths of what it
was.

PROBLEM 6:

What are the units for the rate constant for
this reaction?
1. moles/sec2
2. kJ/mole
3. M4seconds1
4. Rate law constants are unitless.
5. M5 per second
6. (liters per mole-second)6
7. moles per liter
8. moles per second
9. The units are k.

Explanation / Answer

(3) option ( 6 ) is correct i.e., answer is 2 (4).option ( 3 ) is correct , i.e., answer is 3 (5). Given rate r = k[A]2[B]3 A' = A + ( A / 10 ) = 11A / 10 = 1.1 A B ' = B - ( B / 5 ) = 4B / 5 = 0.8 B So, new rate r ' = k [A']2 [B']3                         =k [ 1.1A]2 [0.8B]3                        = k*1.21[A]2 *0.512 [ B]3                       = 0.61952 k [A]2[B]3                       = 0.61952 r (6). Units are M4seconds1

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