Question

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 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

(Reaction A is 2 order, Reaction B is 0 order, Reaction C is 1 order and k= 3.3*10^-3 M^-2s^-1 )

Answer #1

The reaction A+B+C→D+E

Given that; A is 2 order, Reaction B is 0 order, Reaction C is 1 order

Because when the concentration of A is doubles than the rate increase by4 fold.

when the concentration of B is doubles than there is no effect on the rate

when the concentration of C is doubles than the rate increase by 2 fold.

First calculate the value of rate constant ;k as follows:

Rate = k[A]^2[B]^0[C]^1

9.0*10^-5 M/s = k(0.30 M)^2 *(0.30M)^0*(0.30 M)^1

k = 9.0*10^-5 M/s / 0.027 M^-3

k = 3.33*10^-3 M^-2s^-1

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...

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?

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

The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
Order
Integrated Rate Law
Graph
Slope
0
[A]=−kt+[A]0
[A] vs. t
−k
1
ln[A]=−kt+ln[A]0
ln[A] vs. t
−k
2
1[A]= kt+1[A]0
1[A] vs. t
k
Part A
The reactant concentration in a zero-order reaction was
5.00×10−2M after 200 s and
2.50×10−2M after 310 s . What is the rate
constant for this reaction?
Express your answer with...

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...

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...

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...

A certain reaction has an activation energy of 64.0 kJ/mol and a
frequency factor of A1 = 5.70×1012 M−1s−1 .
What is the rate constant, k , of this reaction at 20.0 ∘C
?
Express your answer with the appropriate units. Indicate the
multiplication of units explicitly either with a multiplication dot
(asterisk) or a dash.
Part B
An unknown reaction was observed, and the following data were
collected:
T
(K )
k
(M−1⋅s−1 )
352
109
426
185
Determine...

There are several factors that affect the rate of a reaction.
These factors include temperature, activation energy, steric
factors (orientation), and also collision frequency, which changes
with concentration and phase. All the factors that affect reaction
rate can be summarized in an equation called the Arrhenius
equation:
k=Ae−Ea/RT
where k is the rate constant, A is the
frequency factor, Ea is the activation energy,
R=8.314 J/(mol⋅K) is the universal gas constant, and
T is the absolute temperature.
__________________________________________________
A certain...

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...

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