Question

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?

Answer #1

From the given data we get the order with respect A as 2 ,
comparing 1 and 3 runs, as [A] doubles the rate become 4 times or
2^{2.} Thus we take order with respect to A is 2.

Similarly comparing runs 3 and 4 even after doubling [B] , no change in rate , shows order with respect to B is zero.

Then comparing runs 1 and 2 when [C] increases by 3 times the rate incresed by 3 times, means order with respect to C is one.

Thus the rate expression is written as rate = k
[A]^{2}[B]^{0}[C]

To calculate the rate at different concentration we need to calculaate rate constant k.

By substituting any run values we can evaluate k value.

using run 1 rate = 9.0x10^{-5} = k. (0.3)^{2}
(0.3)

Thus k = 1.0 x10^{-2} / 3

Now Rate when [A] = 0.85 and [B] = [C]= 0.9 wll be

rate = 1.0 x10^{-2}x (0.85)^{2}x (0.9) /3=
0.00216 M/s = 2.16x10^{-3} M/s

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 0.30 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

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:
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+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:
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...

Rate Law: Iodination of
Acetone
Experiment X
trial
initial [A]
initial [B]
Rate (M/s)
#1
1.00 x 10-3
0.25 x
10-3
0.26 x
10-9
#2 1.00 x 10-3
0.50 x
10-3
0.52 x
10-9
#3
1.00 x 10-3
1.00 x
10-3
1.04 x
10-9
#4
2.00 x 10-3
1.00 x
10-3
4.16 x
10-9
#5
3.00 x 10-3
1.00 x
10-3
9.36 x
10-9
#6
4.00 x 10-3
1.00 x
10-3
16.64 x
10-9
Determine the rate law
and calculate...

Determine the rate law for the reaction
2A+3B---> C
[A1] (m)
[B] (m)
Rate (mol/L*s)
0.15
0.30
0.01259
0.30
0.30
0.0159
0.30
0.90
0.0476

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=?)

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

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