Question

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

Answer #1

We can do this in two ways. I'll do it by both ways.

In the first way you can simly use the equation:

r = -dA / dt and solve the values for the concentration of the product and time so:

r = 7.60x10^{-3} - 1x10^{-3} / 40-10 =
2x10^{-4} M/s

However, as the question is an average rate, then, we should do it by the second way, take time intervals, first between 10 and 20, 20 and 30, 30 and 40, and at the end, we'll take the average of those values, and then, compare to the previously obtained:

r_{1} = 4x10^{-3} - 1x10^{-3} / 20-10 =
3x10^{-4} M/s

r_{2} = 5.8x10^{-3} - 4x10^{-3} / 30-20
= 1.8x10^{-4} M/s

r_{3} = 7x10^{-3} - 5.8x10^{-3} / 40-30
= 1.2x10^{-4} M/s

r = (3+1.8+1.2)x10^{-4} / 3 = 2x10^{-4} M/s

Both results are the same, so this would be the correct way to follow.

Hope this helps

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...

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
0.10
0.10
0.10
3.0×10−5
2
0.10
0.10
0.30
9.0×10−5
3
0.20
0.10
0.10
1.2×10−4
4
0.20
0.20
0.10
1.2×10−4
Part A
What is the reaction order with respect to A?
Part B
What is the reaction order with respect to B?
Part C
What is the reaction order...

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...

determine the initial rate for a reaction that starts with 0.85
M of reagent A and 0.70 M of reagents B and C? Express your answer
to two significant figures and include the appropriate units.
Indicate the multiplication of units explicitly either with a
multiplication dot or a dash.
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...

For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate
was measured for various initial concentrations of reactants. The
following data were collected:
Trial
[A][A]
(MM)
[B][B]
(MM)
[C][C]
(MM)
Initial rate
(M/sM/s)
1
0.10
0.10
0.10
3.0×10−5
2
0.10
0.10
0.30
9.0×10−5
3
0.20
0.10
0.10
1.2×10−4
4
0.20
0.20
0.10
1.2×10−4
Question 1:
Given the data calculated in Parts A, B, C, and D,
determine the initial rate for a reaction that starts with 0.65 MM
of reagent AA and...

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 Given the data calculated in Parts A, B, C,
and D, determine the initial rate for a reaction that starts with
0.85 M of reagent A and 0.90 M of reagents B and C?

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.

Consider the following data showing the initial rate of a
reaction (A→products) at several different concentrations of A.
[A](M)
Initial Rate (M/s)
0.15
6.87×10−3
0.30
1.37×10−2
0.60
2.75×10−2
What is the rate law for this reaction?
Rate = k[A]3
Rate = k[A]
Rate = k
Rate = k[A]2
2.)
Consider the following data showing the initial rate of a
reaction (A→products) at several different concentrations of A.
[A](M)
Initial Rate (M/s)
0.15
2.75×10−2
0.30
2.75×10−2
0.60
2.75×10−2
What is the...

Consider the following data showing the initial rate of a reaction
at several different concentrations of A.
[A](M)
0.15
0.30
0.60
Initial Rate (M/s)
0.026
0.207
1.655
What is the order of the reaction? Express as an
integer.
What is the rate law?
Estimate the value of the rate constant, k.

In a series of experiments summarised in the table below, the
initial concentrations of reactants A and B are varied and the
initial rate determined (concentrations are in units of M and the
rates in M s -1). Select the correct rate law for the
reaction.
Experiment
Initial [A]
Initial [B]
Initial Rate
1
0.15
0.12
0.10
2
0.15
0.24
0.40
3
0.45
0.24
0.40
A.
R = k[B]
B.
R = k[A][B]
C.
R = k[B]2
D.
R =...

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