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] |
B] |
[C] |
M/s) |

1 |
0.30 |
0.30 |
0.30 |
9.0×10 |

2 |
0.30 |
0.30 |
0.90 |
2.7×10 |

3 |
0.60 |
0.30 |
0.30 |
3.6×10 |

4 |
0.60 |
0.60 |
0.30 |
3.6×10 |

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 units explicitly either with a multiplication dot or a dash

Answer #1

Answer: Here first we have to calculate the order of the reaction .

Now considering equation 1 and 3 we get :

9.0 * 10^{-5}/3.6 * 10^{-4} = [0.30/0.60]
^{m}

1/4 = 1/2]^{m}

now we get the value of m is 2 .

now consedering data 3 and 4 we get

3.6 * 10^{-4} / 3.6
* 10^{-4} = 1/2]^{n}

1=
1/2]^{n}

hence vale of n is 0

Now we can use the formula to calculate the value of K

from data 4: 3.6 *
10^{-4} = K [ 0.60]^{2}

And we get rate constant
value 10^{-3}

Hence the required answer
is 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

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+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+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...

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?

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...

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 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.

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...

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