Question
In: Chemistry
How to calculate the reaction orders (using experimental data) and write the rate law for a...
How to calculate the reaction orders (using experimental data) and write the rate law for a reaction
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Using the data in the table, calculate the rate constant of this reaction.
Using the data in the table, calculate the rate constant of this
reaction.
A+B⟶C+DA+B⟶C+D
Trial
[?] (?)[A] (M)
[?] (?)[B] (M)
Rate (M/s)
1
0.290
0.240
0.0197
2
0.290
0.528
0.0953
3
0.522
0.240
0.0355
?=
Units=
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
Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall...
Given the following data and using Hess’ Law, Calculate change
in Enthalpy for the reaction
Overall reaction : CH4(g) + 2 O2 (g) ------> CO2(g) +
2H2O(l)
2H2O(l) ------> 2H2O(g) ∆H = 88 kJ
CH4(g) + 2 O2 (g) ------> CO2(g) + 2H2O(g) ------> 2O(g)
∆H = -802 kJ
Given the following data and using Hess’ Law, Calculate change in Enthalpy for the reaction Overall...
Given the following data and using Hess’ Law, Calculate change
in Enthalpy for the reaction Overall reaction : NO(g) + O (g)
------? NO2(g)
2O3(g) ------? 3O2(g) ?H = - 427 kJ
O2(g) ------? 2O(g) ?H = 495 kJ
NO(g) + O3 (g) ------? NO2 (g) + O2 (g) ?H = - 199 kJ
Find the rate law expression and the rate law constant for the reaction whose data is...
Find the rate law expression and the rate law constant for the
reaction whose data is in the table below.
Trial
[X]
[Y]
Rate
1
2.0
2.0
2.5 x 10—6
2
2.0
6.0
2.25 x 10—5
3
4.0
2.0
2.0 x 10—5
b. Calculate the rate of the reaction described in part a) when
[X] = 0.25 mol/L and [Y] = 6.0 mol/L.
For this important smog reaction the experimental rate law is r=kexp [NO]^2[O2]. a.) Show that the...
For this important smog reaction the experimental rate law is
r=kexp [NO]^2[O2]. a.) Show that the following
mechanism is consistent with the rate law and identify keep
proposed mechanism. NO+NO<--> N2O2 fast k1/k-1 N2O2+O--> 2
NO2 slow k2
b.) What is the function of N2O2 and how do you
know?
c.)What is the difference between a catalyst and
an intermediate ?
d.) Activation energies are: 82(r1), 205(r-1, and
82(r2) kJ/mol. If the Arrhenius pre-exponential factors all
approximately the same what...
Calculate the enthalpy of reaction for the following reaction using Hess's Law and the equations provided...
Calculate the enthalpy of reaction for the following reaction
using Hess's Law and the equations provided below.
Target Reaction: Sr(s)+C(graphite)+1 1/2 O2(g) ----->
SrCO3(s) H(degrees)=?
C(Graphite)+ O2(g)-----> CO2(g)
H(degrees)= -349kJ
Sr(s)+ 1/2 O2(G)-------> SrO(s) H(degrees)=
-592kJ
SrO(s)+CO2(g)-------> SrCo3(s)
H(degrees)= -234kJ
1. Based on your experimental determined rate law for the reaction of crystal violet and hydroxide ion, how would doubling the concentration of crystal violet affect the reaction rate?
Trial 1
Time
Trans
A=2-log %T
Ln(A)
1/A
1:57
19.0
0.721
-0.327
1.39
2:52
22.0
0.658
-0.419
1.52
3:51
24.5
0.611
-0.493
1.64
4:54
27.3
0.564
-0.573
1.77
5:53
29.7
0.527
-0.641
1.90
6:54
33.6
0.474
-0.747
2.11
7:55
36.2
0.441
-0.819
2.27
8:54
40.0
0.398
-0.921
2.51
9:52
40.5
0.393
-0.934
2.54
10:53
45.3
0.344
-1.07
2.91
11:58
47.7
0.321
-1.14
3.12
13:02
52.2
0.280
-1.27
3.57
14:02
55.3
0.257
-1.36
3.89
14:59
56.0
0.252
-1.38
3.97
15:59
59.4...
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [A]...
Using the data in the table, calculate the rate constant of this
reaction.
A+B⟶C+D
Trial
[A] (M)
[B] (M)
Rate (M/s)
1
0.280
0.240
0.0160
2
0.280
0.576
0.0922
3
0.504
0.240
0.0288
k=
Units
Using the data in the table, calculate the rate constant of this reaction. A+B⟶C+D Trial [?]...
Using the data in the table, calculate the rate constant of this
reaction.
A+B⟶C+D
Trial
[?] (?)
[?] (?)
Rate (M/s)
1
0.350
0.300
0.0161
2
0.350
0.750
0.101
3
0.490
0.300
0.0225
k= _________? Mention the unit as well
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