Question

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.

Answer #1

rate of disappearance, -r= K[X]^{m} [y]^{n}

m, n are ordes of reaction with respect to [X] and [Y] respectively. K is the rate constant

given 0.127= K[0.2]^{m} [0.3]^{n}
(1)

also given 0.509 =K[0.4]^{m}
[0.3]^{n} (2)

Eq.2/ Eq.1 give

0.509/0.127= [2]^{m}

2^{m}=4, m=2

It is mentioned 0.254 =K[0.2]^{m}
[0.6]^{n } (3)

Eq.3/Eq.2 gives 2= 2^{n}

n=1

so the rate expresion becomes -r =K[X]^{2}
[Y]^{1}

from Eq.1 0.053= K[0.1]^{2} [0.5]1

K= 0.053/0.005 =10.6 /M^{2}.s

so the rate expression becomes -r = 10.6 [X]^{2} [Y]

at X=0.5M and Y=0.3 M

-r =10.6 [0.5]^{2} [0.3] =0.795 M/s

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

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 ...

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- (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 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...

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

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...

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!

Rate data for the reaction 2 CsF + XeF6 →
Cs2XeF8 were taken. Given the data below,
determine the rate law for the reaction.
Trial [CsF]0
(M)
[XeF6]0 (M)
rate0 (M/min)
1
0.10
0.20
0.0145
2
0.20
0.20
0.0289
3
0.30
0.40
0.0867

For the reaction 2 A + B + 2C → 2 D + 3 E, we obtain the data in
the table below. What is this reaction's rate law (be sure to
calculate the value of k)? What is the reaction rate if each
reactant's concentration is 0.70 M. The temperature is
25oC.
[A]o
[B]o
[C]o
rate, vo (M s-1)
0.25
0.20
0.10
0.20
0.25
0.40
0.20
0.40
0.25
0.40
0.40
0.80
0.50
0.40
0.40
0.80
1.00
0.40
1.00
2.00...

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