Question
In: Chemistry
The data shown below were collected for the following second-order reaction: Cl(g)+H2(g)→HCl(g)+H(g)Cl(g)+H2(g)→HCl(g)+H(g) Temperature (K)(K) Rate Constant...
The data shown below were collected for the following
second-order reaction:
Cl(g)+H2(g)→HCl(g)+H(g)Cl(g)+H2(g)→HCl(g)+H(g)
| Temperature (K)(K) | Rate Constant (L/mol⋅s)(L/mol⋅s) |
| 90 | 0.00357 |
| 100 | 0.0773 |
| 110 | 0.956 |
| 120 | 7.781 |
A)Use an Arrhenius plot to determine the activation barrier for the reaction
B)Use an Arrhenius plot to determine the frequency factor for the reaction.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
Part A Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Rate law: k[H]^2 k= 6.4*10^-9 (mol*s) at 500 K...
Part A
Consider the second-order reaction:
2HI(g)→H2(g)+I2(g)
Rate law: k[H]^2
k= 6.4*10^-9 (mol*s) at 500 K
Initial rate = 1.6 * 10^-7 mol (l*s)
What will be the concentration of HI after t =
3.65×1010 s ([HI]t) for a reaction starting
under this condition?
Part B
In a study of the decomposition of the compound X via the
reaction
X(g)⇌Y(g)+Z(g)
the following concentration-time data were collected:
Time (min)
[X](M)
0
0.467
1
0.267
2
0.187
3
0.144
4
0.117
5...
For the elementary gas phase reaction H+C2H4 ®C2H5, the second-order rate constant varies with temperature in...
For the elementary gas phase reaction
H+C2H4 ®C2H5, the
second-order rate constant
varies with temperature in the following way:
T /
K 198 298 400 511 604
1012
k/(cm3molecule-1s-1) 0.20 1.13 2.83 4.27 7.69
a) Use the data to calculate the activation
energy, Ea, and the pre-exponential factor, A, for the
reaction.
b) The simple collision theory of bimolecular
reactions yields the following expression for the rate
constant:
k = (8kT/p m)1/2
sexp(-Ea/RT)
where mis the reduced mass of the reactants and s is the
reaction cross section.
i) Interpret...
The equilibrium constant (Kp) for the reaction below is 4.40 at 2000. K. H2(g) + CO2(g)...
The equilibrium constant
(Kp) for the reaction
below is 4.40 at 2000. K.
H2(g) + CO2(g) ⇌
H2O(g) + CO(g)
Calculate
Δ
G
o
for the reaction.
kJ/mol
Calculate
Δ
G for the reaction when the partial pressures
are
PH2 = 0.22
atm,
PCO2 = 0.72
atm,
PH2O = 0.66 atm,
and
PCO = 1.16 atm.
The gas phase reaction H2 + I2 --> 2HI is second order. Its rate constant at...
The gas phase reaction H2 + I2 --> 2HI is second order. Its
rate constant at 400 C is 0.0243 dm3/mol s. Calculate delta H,
delta S, delta G and the pre-exponential at this temperature.
Assume that delta H is constant over this temperature range.
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) <----->H2(g) +...
The equilibrium constant, K, for the following reaction is
1.80×10-2 at 698
K.
2HI(g)
<----->H2(g) +
I2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
698 K contains 0.322 M
HI, 4.32×10-2 M
H2 and
4.32×10-2 M
I2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if
3.12×10-2 mol of
I2(g) is added to the flask?
[HI]
=
M
[H2]
=
M
[I2]
=
M
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) <----><H2(g) +...
The equilibrium constant, K, for the following reaction is
1.80×10-2 at 698
K.
2HI(g)
<----><H2(g) +
I2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
698 K contains 0.307 M
HI,
4.13×10-2 M
H2 and
4.13×10-2 M
I2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if
0.173 mol of HI(g) is added to
the flask?
[HI]
=
M
[H2]
=
M
[I2]
=
M
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) →...
Determine the equilibrium constant for the following reaction at
655 K.
HCN(g) + 2 H2(g) → CH3NH2(g)
ΔH° = -158 kJ; ΔS°= -219.9 J/K. Determine the equilibrium constant
for the following reaction at 655 K.
HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° =
-158 kJ; ΔS°= -219.9 J/K
A. 3.07 × 1011
B.13.0
C. 3.26 × 10-12
D. 3.99 × 1012
E. 2.51 × 10-13
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) ?...
Determine the equilibrium constant for the following reaction at
655 K.
HCN(g) + 2 H2(g) ? CH3NH2(g); ?H
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) →...
Determine the equilibrium constant for the following reaction at
655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9
J/K
Determine the equilibrium constant for the following reaction at 549 K. CH2O(g) + 2 H2(g) →...
Determine the equilibrium constant for the following reaction at
549 K. CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH° = -94.9 kJ; ΔS°=
-224.2 J/K.
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