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:

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} |

4 | 1.00 | 1.00 | 0.50 | 6.0×10^{−4} |

Answer #1

rate= k [A]^{x} [B]^{y} [C]^{z}

from data table

1.5 x 10^-4 =k [0.5]^{x} [0.5]^{y}
[0.5]^{z} ------------->(1)

4.5 x 10^-4 =k [0.5 ]^{x} [1.50]^{y}
[1.50]^{z} ------------->(2)

6.0 x 10^-4 =k [1.00]^{x} [0.5]^{y}
[0.5]^{z} ------------->(3)

6 x 10^-4 =k [1]^{x} [1]^{y} [0.5]^{z}
------------->(4)

by solving 1 and 2

z = 1

by solving 1 and 3

x = 2

by solving 1 and 4

y = 0

rate= k [A]^{2} [B]^{0} [C]^{1}

from (1)

1.5 x 10^-4 =k [0.5]^{2} [0.5]^{0}
[0.5]^{1}------------>(1)

k = 1.2 x 10^-3 M-2 s-1

0.45 *M* of
reagent A and 0.90 *M* of reagents B and C?

initial rate = 1.2 x 10^-3 x ( 0.45 )^2 x 0.90

**initial rate = 2.19 x 10^- 4 M /s**

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:
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...

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...

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?

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 =...

Constants | Periodic Table
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
0.50
0.050
1.5×10−2
2
0.50
0.100
3.0×10−2
3
1.00
0.050
6.0×10−2
Part a
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.
View Available Hint(s)...

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...

17. The initial concentrations or pressures of reactants and
products are given for each of the following systems. Calculate the
reaction quotient and determine the direction in which each system
will proceed to reach equilibrium.
(a) 2NH3 (g) ⇌ N2 (g) + 3H2 (g) Kc = 17; [NH3] = 0.20 M, [N2] =
1.00 M, [H2] = 1.00 M
(b) 2NH3 (g) ⇌ N2 (g) + 3H2 (g) KP = 6.8 × 104 ; initial
pressures: NH3 = 3.0 atm,...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 10 minutes ago

asked 27 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago