Reaction Rates given no dependence of the rate on the concentration of the chemical reactant

1. Rate Law: Zeroeth-Order Reaction
A→B
Rate Law:
0
Rate = k x [A]
B appears at same rate that A
disappears, but the rate is independent
of the concentration of A

2. 0
[A]
[B]
1.50
0.00
Reaction
Begins:
Initial
Concentration
Of A is 1.50 M
K
0.05
M/s
Concentration v Time
A rearranging to B
1.6
1.4
Concentration (M)
Time (s)
1.2
[A]
[B]
1
0.8
0.6
0.4
0.2
0
0
5
10
15
20
time
25
30
35
40

3. Time
[A]
[B]
0
1.50
0.00
1
1.45
0.05
Zeroeth Order Reaction
Rate = k[A]º
1.6
1.4
1.2
[A]
[B]
1
[A] (M)
In first second,
0.05 molar
Reduction in [A]
And 0.05 molar
Increase in [B]
0.8
0.6
0.4
0.2
0
0
5
10
15
20
time (s)
25
30
35
40

4. Time
[A]
[B]
0
1.50
0.00
1
1.45
0.05
2
1.40
0.10
Zeroeth Order Reaction
1.6
1.4
1.2
1
[A] (M)
In second
second, rate is
the same
because
[A] has no effect
on the rate
[A]
[B]
0.8
0.6
0.4
0.2
0
0
5
10
15
20
time (s)
25
30
35
40

5. Time
[A]
[B]
0
1.50
0.00
5
1.25
0.25
10
1.00
0.50
15
0.75
0.75
20
0.50
1.00
25
0.25
1.25
0.00
1.6
1.4
1.2
1.50
A reaction rate
study yielding a
linear relationship
between time and
concentration
indicates a zeroeth
order reaction in
the reactant. This
is uncommon.
1
[A] (M)
30
Zeroeth Order Reaction
[A]
[B]
0.8
0.6
0.4
0.2
0
0
5
10
15
20
25
30
35
40
time (s)
After 30 seconds it is easy to
see the reaction is over.

6. Lower Rate Constant
Zeroeth Order Reaction
1.6
1.4
1.2
[A] (M)
1
[A]
[B]
0.8
0.6
0.4
0.2
0
0
5
10
15
20
25
30
35
40
time (s)
This is the effect of changing
the rate constant to 0.01 M/s.
The reaction is much slower
but the concentration does
not affect the rate.

7. Higher Rate Constant
Zeroeth Order Reaction
1.6
1.4
1.2
[A] (M)
1
[A]
[B]
0.8
0.6
0.4
0.2
0
0
5
10
15
20
25
30
35
40
time (s)
This is the effect of changing
the rate constant to 0.10 M/s.
The reaction is much faster.
Still no concentration effect.