Wired Faculty-
Call Us
+91 8076753736 -
Send us an Email
[email protected]
Thermodynamics
Question
In the conversion of limestone to lime, CaCO3(s) → CaO(s) + CO2(g) the values of ∆Hº and ∆Sº are + 179.1 kJ mol–1 and 160.2 J/K respectively at 298K and 1 bar. Assuming that ∆Hº and ∆Sº do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is
-
1008 K
-
1200 K
-
845 K
-
1118 K
Solution
D.
1118 K
We know, ∆G = ∆H-T∆S
So, lets find the equilibrium temperature, i.e. at which
∆G = 0
∆H-T∆S
T= 179.1 x 1000/160.2
= 1118 K
So, at the temperature above this, the reaction becomes will spontaneous.
Sponsor Area
Some More Questions From Thermodynamics Chapter
From thermodynamic point of view, to which system the animals and plants belong?
What is a state function?
A thermodynamic state function is a quantity
What is reversible process in thermodynamics?
Define irreversible change.
Name the variable that is kept constant in isochoric process and isobaric process.
Give one difference between an isothermal and an adiabatic process.
For the process to occur under adiabatic conditions, the correct condition is
Define internal energy of a system
Define enthalpy.
Mock Test Series
Sponsor Area