Question
In: Chemistry
3. In each of the rate laws given below, determine the overall reaction order. A) rate...
3. In each of the rate laws given below, determine the overall reaction order.
A) rate = k[A]2[B]0
B) rate = k[A]2[B]-1
C) rate = k[A]1[B]3
D) rate = k[A]3[B]-1
E) rate = k[A]3[B]0
4. Consider the following equation with the rate law:
C + D→F + G Rate law = k[C]2[D]1/2
Evaluate each of the following statements as TRUE or FALSE. Show work for each!
A) If the concentration of D is increased by a factor of 4, then the reaction rate will double.
B) If the concentration of C is doubled and the concentration of D is tripled, then the reaction rate will increase by a factor of 6.9.
C) If the concentration of C is increased by a factor of 3 and the concentration of D is decreased by a factor of 4, then the reaction rate will increase by a factor of 4.5.
D) If the concentrations of C and D are doubled, then the reaction rate will triple.
E) If the concentration of C is increased by a factor of 4, then the reaction rate will increase by a factor of 16.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
For the reaction below, A. determine the order of each reactant
For the reaction below,
A. determine the order of each reactant (3 points)
B. the overall order (1 point)
C. the average rate constant (1 points)
using the method of initial rates.
2A + B +C à D + 2E
Experiment
[A]
[B]
[C]
Initial Rate (M/s)
1
1.5
0.50
2.0
5.0 x 10-3
2
0.75
0.50
1.0
2.5 x 10-3
3
0.75
0.50
2.0
5.0 x 10-3
4
1.5
1.00
1.0
2.0 x 10-2
5
1.5
0.50
1.0...
The overall reactions and rate laws for several reactions are given below. Which one of these...
The overall reactions and rate laws for several reactions are
given below. Which one of these represents an elementary step?
A) A + 2B → P rate = k[A]2
B) A + 2B → P rate = k[A][B]
c) 2A → P rate = k[A]
D)A + B + C → P rate = k[A][C]
E) A + B → P rate = k[A][B]
1. What is the overall reaction order for the reaction that has the rate law: Rate...
1. What is the overall reaction order for the reaction that has
the rate law: Rate = k[H2] [NO]2 ?
a. zero
order
b. first
order
c. second
order
d. third
order
2. The first-order decomposition of hydrogen peroxide occurs
according to the equation
2 H2O2(aq) ? 2 H2O(l) +
O2(g)
Using data from a concentration-time study of this reaction,
which plot will produce a straight line?
a.
1/[H2O2] versus time
b.
ln[H2O2] versus time
c.
[H2O2]2 versus time
d. ...
Given the following data collected from experiments, determine the rate law, overall order, and the numerical...
Given the following data collected from experiments, determine
the rate law, overall order, and the numerical value for the rate
constant.
Experiment
[A]
[B]
Initial Rate (M sec^-1)
1
0.250
0.400
0.400
2
0.0500
0.800
0.0320
3
0.0500
0.100
0.00400
3. Given the initial rate data for the reaction A + B –––> C, determine the...
3. Given the initial rate data for the reaction A + B –––> C,
determine the rate expression for the reaction. [A], M [B], M Δ
[C]/ Δ t (initial) M/s 0.215 0.150 5.81 x 10–4 0.215 0.300 1.16 x
10–3 0.430 0.150 2.32 x 10–3 A) (Δ[C]/Δt) = 1.80 x 10–2 M –1 s –1
[A][B] B) (Δ[C]/Δt) = 3.60 x 10–2 M –1 s –1 [A][B] C) (Δ[C]/Δt) =
1.20 x 10–1 M –2 s –1 [A][B]2 D)...
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they...
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
1) The reactant concentration in a zero-order reaction was
6.00×10−2M after 150 sand
3.50×10−2M after 330 s . What is the rate
constant for this reaction? Express your answer with the
appropriate...
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they...
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
a.)
The reactant concentration in a zero-order reaction was
6.00×10−2M after 140 s and
2.00×10−2Mafter 310 s . What is the rate
constant for this reaction?
b.)
What was the initial reactant...
Integrated Rate Laws: Working with Zero Order Reactions Experiments have shown the following reaction to be...
Integrated Rate Laws: Working with Zero Order Reactions
Experiments have shown the following reaction to be zero order with
a rate constant = 2.50 10-1 M/sec. A → B + 2 C If you started with
[A] = 2.600 M, how many minutes until the concentration of A =
2.300 M? .02 Correct: Your answer is correct. minutes How many
minutes until the concentration of C reaches equals
0.899999999999999 M? 1.73 Incorrect: Your answer is incorrect.
minutes
What is the overall order of the reaction below 2 NO(g) + O2(g) → 2 NO2(g)...
What is the overall order of the reaction below
2 NO(g) + O2(g) → 2
NO2(g)
if it proceeds via the following rate expression?
a)
zero-order b)
first-order
c) second-order d)
third-order e)
fourth-order
Using the data listed below, determine the rate law and the rate constant for this reaction...
Using the data listed below, determine the rate law and the rate
constant for this reaction at 60°C with respect to hypochlorite
decomposition.
t (min)
[ClO-] (M)
0
0.950
60
0.941
120
0.932
240
0.915
360
0.898
480
0.882
720
0.851
1080
0.809
1440
0.771
1800
0.736
2160
0.705
2520
0.676
2880
0.649
3600
0.601
4320
0.560
5040
0.524
5760
0.493
6480
0.465
7200
0.440
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