Question
In: Chemistry
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 |
Solutions
Expert Solution
We know that
Go =
Ho -
TSo
Given:
Ho =
-158 kJ = - 158000 J
So =
-219.9 J/K
T = 655 K
So,
Go =
(- 158000 J) - (655 K) (-219.9 J/K)
= - 158000 J + 144034.5 J
= - 13965.5 J
Again,
Go = -
RT lnK
Where K is the equilibirium constant.
So,
- 13965.5 J = - (8.314 J K-1mol-1) (655 K) ln K
13965.5 =
5445.67 ln K
ln K =
13965.5 / 5445.67
ln K =
2.56
K = e
2.56
K = 12.93 =
13
Answer is (B).
queen_honey_blossom answered 3 years agoRelated Solutions
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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
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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
The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) ---> H2(g)...
The equilibrium constant, Kc, for the following reaction is
1.80×10-2 at 698 K.
2HI(g) ---> H2(g) + I2(g)
Calculate the equilibrium concentrations of reactant and
products when 0.384 moles of HI are introduced into a 1.00 L vessel
at 698 K.
[HI] = M
[H2] = M
[I2] = M
The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) -->H2(g) +...
The equilibrium constant, Kc, for the following
reaction is 1.80×10-2 at
698 K.
2HI(g)
-->H2(g) +
I2(g)
Calculate the equilibrium concentrations of reactant and products
when 0.257 moles of HI are
introduced into a 1.00 L vessel at 698
K.
[HI]
=
M
[H2]
=
M
[I2]
=
M
The equilibrium constant, Kc, for the following
reaction is 83.3 at 500 K.
PCl3(g) +
Cl2(g)
-->PCl5(g)
Calculate the equilibrium concentrations of reactant and products
when 0.420 moles of
PCl3 and...
1. Determine the equilibrium constant for the following reaction at (3.950x10^2) K. 2 A(g) + B2(g)...
1. Determine the equilibrium constant for the following reaction
at (3.950x10^2) K.
2 A(g) + B2(g) → 2
AB(s) ΔH° = -(2.2x10^2) kJ; ΔS° =
-(3.988x10^2) J/K
2.
A+ (aq) + BC3- (aq) à
A(BC3)(s) ΔH° f = -64.4 kJ/mol
For the above reaction ΔSsys is ________(positive or negative),
and ΔG is __________ (positive or negative) and the reaction is
_______________ (spontaneous or nonspontaneous) at
600K
3.
Which of the following pairs of reactants will result in a
spontaneous reaction...
The equilibrium constant (Kp) for the following reaction is 4.40 at 2000.K. H2(g) + CO2(g) <=>...
The equilibrium constant (Kp) for the following reaction is 4.40
at 2000.K.
H2(g) + CO2(g) <=>
H2O(g) + CO(g)
a) Calculate Delta Go for the reaction. ____________
KJ/mol
b) Calculate Delta G for the reaction when the partial pressures
are PH2 = 0.28 atm, PCO2 = 0.81 atm,
PH2O = 0.63 atm, and PCO = 1.17 atm.
______________ KJ/mol
Q1)Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) →...
Q1)Determine the equilibrium constant for the following reaction
at 498 K.
2 Hg(g) + O2(g) → 2 HgO(s) ΔH° = -304.2 kJ; ΔS° = -414.2
J/K
a)1.87 × 1010
b)2.31 × 10-22
c)4.33 × 1021
d)8.10 × 1031
e)5.34 × 10-11
Q2) 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)2.51 × 10-13
b)3.99 × 1012
c)3.26 × 10-12
d)13.0
e)3.07 × 1011
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