Question

Assuming the CV initial concentration is 1.2 x 10-5 M, calculate the time required for the concentration to decrease to 40% of the initial value.

Answer #1

Need more information for the problem. Atleast we should know which order of the reaction it is.

For time sake think its First order for which we need K rate constant.

For first order rate equation is ln(Ca/Cao) = -kt => ln(0.4
Cao /Cao) = - kt => - 0.9163 = - kt => **t = 0.9163 /
k**

If you know the rate constant substitute in that you will get time required.

If it is not first order consider taking this n th order
**Ca ^{(1-n)} - Cao^{(1-n)} = (n-1)**
kt where n is order of the reaction, doesnt hold for first
order.

Consider the reaction and the initial concentration and initial
rate data below.
BrO3-(aq) + 5 Br- (aq) + 6 H+(aq) ® 3 Br2 (aq) + 3 H2O (l)
Experiment
[BrO3-], (M)
[Br-],(M)
[H+],(M)
Initial Rate (M/sec)
1
0.10
0.10
0.10
1.2 x 10-3
2
0.20
0.10
0.10
2.4 x 10-3
3
0.10
0.30
0.10
3.5 x 10-3
4
0.20
0.10
0.15
5.4 x 10-3
Determine the rate law for this reaction
What is the overall order of the rate law?...

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acetic acid in the vinegar. A particular sample of vinegar has a pH
of 2.95.
b) The acid-dissociation constant for benzoic acid (C6H5COOH) is
6.3×10−5. Calculate the equilibrium concentration of H3O+ in the
solution if the initial concentration of C6H5COOH is
6.2×10−2 M .
c) Calculate the equilibrium concentration of C6H5COO− in the
solution if the initial concentration of C6H5COOH is
6.2×10−2 M ....

Benzoic acid, C6H5CO2H, is a weak acid (Ka=6.3x10^-5). Calculate
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2.54

The acid-dissociation constant for benzoic acid (C6H5COOH) is
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Part A Calculate the equilibrium concentration of H3O+ in the
solution if the initial concentration of C6H5COOH is 6.3×10−2 M .
Express your answer using two significant figures.
Part B Calculate the equilibrium concentration of C6H5COO− in
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.
Part C Calculate the equilibrium concentration of C6H5COOH in
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. Express...

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. Express your answer using two significant figures. Part B
Calculate the equilibrium concentration of C6H5COO− in the solution
if the initial concentration of C6H5COOH is 6.3×10−2 M . Part C
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Express your answer using two significant figures.
HC2H3O2 =
M
SubmitMy AnswersGive
Up

The acid-dissociation constant for benzoic acid (C6H5COOH) is
6.3×10−5.
Part A
Calculate the equilibrium concentration of H3O+ in the solution
if the initial concentration of C6H5COOH is 6.6×10−2 M
.
Express your answer using two significant figures.
[H3O+] =
M
SubmitRequest Answer
Part B
Calculate the equilibrium concentration of C6H5COO− in the
solution if the initial concentration of C6H5COOH is
6.6×10−2 M .
Express your answer using two significant figures.
[C6H5COO−] =
M
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Rate Law: Iodination of
Acetone
Experiment X
trial
initial [A]
initial [B]
Rate (M/s)
#1
1.00 x 10-3
0.25 x
10-3
0.26 x
10-9
#2 1.00 x 10-3
0.50 x
10-3
0.52 x
10-9
#3
1.00 x 10-3
1.00 x
10-3
1.04 x
10-9
#4
2.00 x 10-3
1.00 x
10-3
4.16 x
10-9
#5
3.00 x 10-3
1.00 x
10-3
9.36 x
10-9
#6
4.00 x 10-3
1.00 x
10-3
16.64 x
10-9
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