Question

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

Answer #1

Let the rate law for the reaction be,

rate = k[A]^x.[B]^y

with,

k being the rate constant

x and y be order with respect to [A] and [B]

compare trial 1 and 2, [A] is constant and gets cancelled out,

rate1/rate2 = 0.0170/0.0979 = (0.33/0.792)^y

y = 2

compare trial 1 and 3, [B] is same and gets cancelled out,

rate1/rate3 = (0.0170/0.0204) = (0.230/0.276)^x

x = 1

So the rate law becomes,

rate = k[A].[B]^2

Now take trial 1,

k = 0.0170/(0.230) x (0.330)^2 = 0.68 1/M^2.s

Is the rate constant.

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

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.

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...

For the reaction A+B+C→D+E, the initial reaction rate was
measured for various initial concentrations of reactants. The
following data were collected:
Given the data calculated in Parts A, B, C, and D, determine the
initial rate for a reaction that starts with 0.45 M of
reagent A and 0.90 M of reagents B and C?
Trial
[A]
(M)
[B]
(M)
[C]
(M)
Initial rate
(M/s)
1
0.50
0.50
0.50
1.5×10−4
2
0.50
0.50
1.50
4.5×10−4
3
1.00
0.50
0.50
6.0×10−4...

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

I cannot seem to answer this question correctly. Could you show
me step by step how to work this?
Using the given data, calculate the rate constant of this
reaction.
A+B ------
C+D
Trial
A(M)
(B)M (C)
1 0.330 0.370 0.0135
2
0.330 0.999
0.0984
3
0.495
0.370 0.0203
K=

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→D+E, the initial reaction rate was
measured for various initial concentrations of reactants. The
following data were collected:
Trial
[A]
(M)
B]
(M)
[C]
(M)
Initial rate
(M/s)
1
0.30
0.30
0.30
9.0×10−5
2
0.30
0.30
0.90
2.7×10−4
3
0.60
0.30
0.30
3.6×10−4
4
0.60
0.60
0.30
3.6×10−4
rate=k[A]^m[B]^n
What is the value of the rate constant k for this reaction?
Express your answer to two significant figures and include the
appropriate units. Indicate the multiplication of...

REACTION A + B + C ---> Products
Trial
[A](M)
[B](M)
[C](M)
Rate(M/s)
1
1.0
1.0
0.010
1.0E-4
2
1.0
2.0
0.010
4.0E-4
3
1.0
1.0
0.020
2.0E-4
4
2.0
1.0
0.010
2.0E-4
Using the data in the table and the rate law below, identify the
reaction order with respect to each reactant.
Rate = k[A]m[B]n[C]p
(I need to find m=?, n=?, and p=?)

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