Question
Consider the reaction X + Y → Z From the data in the table, obtained at...
Consider the reaction X + Y → Z From the data in the table, obtained at 360 K,
(a) determine the overall order of the reaction 2 Initial Rate of Disappearance of X (M/s) [X] (M) [Y](M)
(b) determine the initial rate of disappearance of X when the concentration of X is 0.40 M and that of Y is 0.20 M.
initial rate of disappearance of X (m/s) [X] (M) [Y](M)
.053 .1 .5
.127 .2 .3
1.02 .4 .6
.254 .2 .6
.509 .4 .3
Homework Answers
Answer #1
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Similar Questions
Consider the reaction X + Y → Z From the data in the table, obtained at...
Consider the reaction X + Y → Z From the data in the table,
obtained at 360 K, (a) determine the overall order of the reaction
Initial Rate of Disappearance of X (M/s) [X] (M) [Y](M) 0.053 0.10
0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30
(b) determine the initial rate of disappearance of X when the
concentration of X is 0.50 M and that of Y is 0.30 M.
Consider the reaction: X + Y -> Z. FRom the data below, determine the Rate when...
Consider the reaction: X + Y -> Z. FRom the data below,
determine the Rate when [X] = 0.50M and [Y] = 0.25M.
Rate (M/s) [X](M) [Y](M)
0.053 ------0.10----0.50
0.127-------0.20----0.30
1.02---------0.40----0.60
0.254-------0.20----0.60
0.509-------0.40-----0.30
A + B -> C initial rate data: [A] .10, .20, .40, .20, .40 [B] .50,...
A + B -> C
initial rate data:
[A]
.10, .20, .40, .20, .40
[B]
.50, .30, .60, .60, .30
initial rate (M/s)
.053, .127, 1.02, .254, .509
determine a)the basic rate law for this reaction b)
the rate constant of reaction
For the reaction, A(g) + B(g) => 2 C(g), the following data were obtained at constant...
For the reaction, A(g) + B(g) => 2 C(g), the following data
were obtained at constant temperature.
Experiment
Initial [A], mol/L
Initial [B], mol/L
Initial Rate, M/min
1
0.10
0.10
2 x 10-4
2
0.30
0.30
5.4 x 10-3
3
0.10
0.30
1.8 x 10-3
4
0.20
0.40
6.4 x 10-3
Which of the following is the correct rate law for the
reaction?
1.
Rate = k[A][B]
2.
Rate = k[A]2[B]
3.
Rate = k[A]2[B]2
4.
Rate = k[A]
5....
Consider the reaction and the initial concentration and initial rate data below. BrO3-(aq) + 5 Br-...
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?...
Consider the gas-phase reaction between nitric oxide and bromine at 273 ?C 2NO(g)+Br2(g)?2NOBr(g). The following data...
Consider the gas-phase reaction between nitric oxide and bromine
at 273 ?C
2NO(g)+Br2(g)?2NOBr(g).
The following data for the initial rate of appearance of NOBr were
obtained:
Experiment
[NO](M)
[Br2](M)
Initial Rate of Appearance of NOBr(M/s)
1
0.10
0.20
24
2
0.25
0.20
150
3
0.10
0.50
60
4
0.35
0.50
735
rate=k[NO]2[Br2]
Calculate the average value of the rate constant for the
appearance of NOBr from the four data sets.
k= _______ M^-2s^-1
What is the rate of disappearance of...
14.37 Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following...
14.37
Consider the gas-phase reaction
between nitric oxide and bromine at 273 ∘C
2NO(g)+Br2(g)→2NOBr(g).
The following data for the initial rate of appearance of NOBr were
obtained:
Experiment
[NO](M)
[Br2](M)
Initial Rate of Appearance ofNOBr(M/s)
1
0.10
0.20
24
2
0.25
0.20
150
3
0.10
0.50
60
4
0.35
0.50
735
Part A
Determine the rate law.
Determine the rate law.
a.
rate=k[NO]2[Br2]
b.
rate=k[NO][Br2]
c.
rate=k[NO]2[Br2]2
d. rate=k[NO][Br2]2
Part B
Calculate the average value of the rate constant for...
For the reaction A + B + C → products, the following initial-rate data were obtained....
For the reaction A + B + C → products, the following
initial-rate data were obtained.
[A]0 (mol/L)
[B]0 (mol/L)
[C]0 (mol/L)
Initial Rate (mol/(L · s))
0.40
0.40
0.20
0.0160
0.20
0.40
0.40
0.0080
0.60
0.10
0.20
0.0015
0.20
0.10
0.20
0.0005
0.20
0.20
0.40
0.0020
What are the reaction orders with respect to A, B, and C,
respectively?
A.
0, 2, 1
B.
1, 1, 1
C.
1, 2, 0
D.
1, 2, 1
E.
0, 1, 1
Consider the gas-phase reaction between nitric oxide and bromine at 273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data...
Consider the gas-phase reaction between nitric oxide and bromine at
273 ∘C
2NO(g)+Br2(g)→2NOBr(g).
The following data for the initial rate of appearance of NOBr were
obtained:
Experiment
[NO](M)
[Br2](M)
Initial Rate of Appearance ofNOBr(M/s)
1
0.10
0.20
24
2
0.25
0.20
150
3
0.10
0.50
60
4
0.35
0.50
735
Part D
What is the rate of disappearance of Br2 when [NO]=
7.6×10−2 M and [Br2]=0.21 M ?
Please help with part d!
The following data were obtained for the chemical reaction: A + B ---> products Exp. Initial...
The following data were obtained for the chemical reaction: A +
B ---> products
Exp.
Initial A
(mol/L)
Initial B
(mol/L)
Init. Rate of Formation
of products (M s-1)
1
0.040
0.040
9.6 x 10-6
2
0.080
0.040
1.92 x 10-5
3
0.080
0.020
9.6 x 10-6
(a) Determine the rate law for this reaction.
(b) Find the rate constant.
(c) What is the initial rate of reaction when [A]o =
0.12 M and [B]o = 0.015
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