Thermodynamics ...

For a reversible reaction,
X (g) + 3Y (g) ⇌ 2Z(g); ∆H = - 40 kJ, the standard entropies of X ,Y and Z are 60, 40 and 50 JK^-1 mol^-1 respectively. The temperature at which the above reaction attains equilibrium is about

The decomposition of limestone
CaCO₃ (g) ⇌ CaO(s) + CO₂ (g)
is non-spontaneous at 298 K. The ∆H° and ∆S° values for the reaction are 76.0 kJ and 60 JK^-1 respectively. At what temperature the decomposition becomes spontaneous ?

Identify the correct statement regarding a spontaneous process.

In conversion of limestone to lime,
CaCO₃ (s) → CaO(s) + CO₂ (g )
the values of ∆H° and ∆S °are + 179.1 kJ mol^-1 and 160.2 J/K respectively at 298 K and 1 bar. Assuming that ∆H° and ∆S ° do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are - 382.64 kJ mol^-1 and - 145.6 JK^-1 mol^-1, respectively. Standard Gibbs energy change for the same reaction at 298 K is

Which of the following is correct for the reaction ∆H = +ve and ∆S = +ve?

What is the relation between E° and K ?

A schematic plot of In K_eq versus inverse of temperature for a reaction is shown below

The enthalpy change for the transition of liquid water to steam is 40.8 kJ per mol at 100°C. The entropy change for the process will be

If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point, then