MolSynapse
question bank
All chapters
NEET
JEE
Practice
MolSynapse
/
Question bank
/
Chemical Equilibrium
/
Thermodynamics of equilibrium: van't Hoff equation
JEE Main level
Numerical answer
Difficulty 2 of 3
ce140
Take
R
=
8.314
J
mo
l
−
1
K
−
1
. A reaction has
K
=
5.0
×
1
0
−
3
at
350
K
. Calculate
Δ
G
∘
in
kJ
mo
l
−
1
(one decimal).
Numerical answer type, answer in kJ/mol, tolerance 0.1.
Answer: 15.4 kJ/mol
Δ
G
∘
=
−
RT
ln
K
=
−
(
8.314
)
(
350
)
ln
(
5.0
×
1
0
−
3
)
/1000
=
−
(
2909.9
)
(
−
5.2983
)
/1000
=
+
15.418
kJ
mo
l
−
1
. It is positive because
K
<
1
.
Practice Chemical Equilibrium
More on Thermodynamics of equilibrium: van't Hoff equation
Previous question
Next question
More questions on Thermodynamics of equilibrium: van't Hoff equation
Take R = 8.314 J mol^-1 K^-1. For a gas-phase reaction at 400 K, K = 50. The reaction quotient of a mixture is Q = 5.0. The Gibbs energy cha...
JEE Main level
Take R = 8.314 J mol^-1 K^-1. A reaction has K = 1.5 x 10^-3 at 400 K and K = 4.8 x 10^-2 at 450 K. Assuming Delta H deg is independent of t...
JEE Main level
Take R = 8.314 J mol^-1 K^-1. For a reaction, K = 0.25 at 350 K and Delta H deg = +40.0 kJ mol^-1 (constant). Calculate K at 400 K (two deci...
JEE Main level
For the decomposition of a carbonate, Delta H deg = +178.0 kJ mol^-1 and Delta S deg = +165 J mol^-1 K^-1, both assumed independent of tempe...
JEE Main level
The reaction 2SO2(g) + O2(g) <=> 2SO3(g) has Delta H deg = -198 kJ per mole of reaction. Which statements are correct?
JEE Main level
Take R = 8.314 J mol^-1 K^-1. A reaction has Delta G deg = +9.0 kJ mol^-1 at 300 K. Which statements are correct?
JEE Main level