Question

Using the given data, determine the rate constant of this reaction: A+2B ----> C+D

Trial [A] (M) [B] (M) Rate (M/s)

1 0.320 0.300 0.0121

2 0.320 0.600 0.0121

3 0.640 0.300 0.0484

Answer #1

Using the given data, calculate the rate constant of this
reaction: A+B ---> C+D
Trial
[A] (M) [B}
(M)
Rate (M/s)
1
0.230
0.330
0.0170
2
0.230
0.792
0.0979
3
0.276 0.330
0.0204

using the given data, calculate the rate constant of this
reaction. A+B yields C+D Trial: 1,2,3 [A](M): 0.370, 0.370, 0.592
[B](M):0.340, 0.782, 0.340 Rate(M/s): 0.0210, 0.111, 0.0336 K= ?
Please provide the units as well. Please show work so I can
understand the problem.

Using the given data, calculate the rate constant of this
reaction. A+B yield C+D
A [M] B [M] rate
.370, .340 .0210
.370 .782 .111
.592 .340 .0336
STRATEGY: 1. Determine the rate law. 2. Solve the rate law for k
and calculate the k value.

Given the following data collected from experiments, determine
the rate law, overall order, and the numerical value for the rate
constant.
Experiement
[A]
[B]
Initial Rate (M min ^-1)
1
0.200
0.300
0.300
2
0.800
0.300
4.80
3
0.200
0.600
2.40

With the experimental data given for the kinetic study of the
reaction
A + 2B == AB2, answer the following two questions
Experiment [A] 0 M [B] 0 M Initial velocity formation rate of
AB2 (M / min)
1 0.5 1.5 4.2x10-3
2 1.5 1.5 1.3x10-2
3 3.0 3.0 5.2 x10-2
11.-Determine the law of speed for the reaction
Answer: ___________________________
12.- Calculate the value of the kinetic constant
Answer: __________________

Consider the reaction
A+2B⇌C
whose rate at 25 ∘C was measured using three different sets of
initial concentrations as listed in the following table:
Calculate the initial rate for the formation of C at 25 ∘C, if
[A]=0.50M and [B]=0.075M.
Express your answer to two significant figures and include the
appropriate units.
Trial
[A]
(M)
[B]
(M)
Rate
(M/s)
1
0.35
0.010
1.5×10−3
2
0.35
0.020
2.9×10−3
3
0.70
0.010
5.9×10−3

Using the given data, determine the rate constant of this
reaction. _[A]_______[B]________Rate 1) 0.260____0.270______0.0194
2) 0.260____0.540______0.0194 3) 0.520____0.270______0.0776

Consider the reaction
A+2B⇌C
whose rate at 25 ∘C was measured using three different sets of
initial concentrations as listed in the following table:
Trial
[A]
(M)
[B]
(M)
Rate
(M/s)
1
0.15
0.010
2.7×10−4
2
0.15
0.020
5.4×10−4
3
0.30
0.010
1.1×10−3
Calculate the initial rate for the formation of C at 25 ∘C, if
[A]=0.50M and [B]=0.075M.
Express your answer to two significant figures and include the
appropriate units.

Given the initial rate data for the
reaction A + B → C, determine the rate expression for the
reaction.
[A], M
[B], M
Δ[C]/Δt (initial) M/s
0.0500
0.160
2.24 ´ 10-3
0.0750
0.160
3.36 ´ 10-3
0.0750
0.272
9.72 ´ 10-3

For the reaction A + B → C the following data is obtained:
Trial
[A]
[B]
RateA
1
0.2 M
0.2 M
1.2 x 10-3 M/min
2
0.1 M
0.2 M
6.0 x 10-4 M/min
3
0.2 M
0.1 M
1.2 x 10-3 M/min
After you determine the rate law, what is the value of the rate
constant for the reaction using the given units? If you choose to
enter your answer in scientific notation you must enter it this...

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