Chemical Reaction Equilibrium - Thermodynamics - Chemical Engineering Previous Year Questions

A gaseous system contains H₂, I₂, and HI, which participate in the gas-phase reaction
2 HI ⇌ H₂ + I₂
At a state of reaction equilibrium, the number of thermodynamic degrees of freedom is ______

Match the following

Group 1	Group 2
P. \( \left( \frac{\partial G}{\partial n} \right)_{T,P,n_j} \)	I. Arrhenius equation
Q. \( \left( \frac{\partial G}{\partial n} \right)_{S,V,n_j} \)	II. Reaction equilibrium constant
R. \( \exp \left( \frac{-\Delta G_{reaction}^{0}}{RT} \right) \)	III. Chemical potential
S. \( \sum (n_i d\mu_i)_{T,p} = 0 \)	IV. Gibbs-Duhem equation

Carbon monoxide (CO) reacts with hydrogen sulphide (H₂S) at a constant temperature of 800 K and a constant pressure of 2 bar as:
CO + H₂S ⇌ COS + H₂
The Gibbs free energy of the reaction ΔG°_rxn = 22972.3 J/mol and universal gas constant R=8.314 J/(mol K). Both the reactants and products can be assumed to be ideal gases. If initially only 4 mol of H₂S and 1 mol of CO are present, the extent of the reaction (in mol) at equilibrium is ______ (rounded off to two decimal places).

The heat of combustion of methane, carbon monoxide and hydrogen are \(P\), \(Q\) and \(R\) respectively. For the reaction below,
\[ CH_4 + H_2O \longrightarrow CO + 3H_2 \]
the heat of reaction is given by

For a reversible endothermic chemical reaction with constant heat of reaction over the operating temperature range, \( K \) is the thermodynamic equilibrium constant. Which one of the following figures shows the CORRECT dependence of \( K \) on temperature \( T \)?

Methanol is formed by the following gas phase homogeneous reaction:
CO (g) + 2H₂ (g) ⇌ CH₃OH (g)
The standard Gibbs free energies of formation at 298 K for CO and CH₃OH are −137 kJ mol⁻¹ and −162 kJ mol⁻¹, respectively. The value of universal gas constant is 8.314 J mol⁻¹ K⁻¹. The equilibrium constant for the given reaction at 298 K is ______ × 10⁴ (rounded off to one decimal place).