Find the correct equation

• E₂ - E₁ - H₂ + H₁ = n₂RT - n₁RT

• E₂ - E₁ - H₂ - H₁ = n₂RT - n₁RT

• H₂ - H₁ - E₂ + E₁ = n₂RT - n₁RT

• H₂ - H₁ - E₂ - E₁ = n₂RT - n₁RT

Assuming enthalpy of combustion of hydrogen at 273 K is -286 kJ and enthalpy of fusion of ice at the same temperature to be +6.0 kJ, calculate enthalpy change during formation of 100 g of ice.

• +1622 kJ

• - 1622 kJ

• +292 kJ

• - 292 kJ

83.

For which among the following reactions, change in entropy is less than zero?

• Sublimation of iodine

• Dissociation of hydrogen

• Formation of water

• Thermal decomposition of calcium carbonate

Which among the following is a feature of adiabatic expansion?

• $∆$V < 0

• $∆$U < 0

• $∆$U > 0

• $∆$T = 0

What is the amount of work done when two moles of ideal gas is compressed from a volume of 1m³ to 10 dm³ at 300 K against a pressure of 100 kPa?

• 99 kJ

• -99kJ

• 114.9 kJ

• -114.9 kJ

The work done during combustion of 9 × 10^-2 kg of ethane, C₂H₆ (g) at 300 K is (Given R = 8.314 J deg^-1 mol^-1, atomic mass C = 12, H= 1).

• 6.236 kJ

• -6.236 kJ

• 18.71 kJ

• -18.71 kJ

The first law of thermodynamics for isothermal process is

• q = -W

• $∆$U = W

• $∆$U = q_v

• $∆$U = -q_v

Identify the invalid equation

• $∆\mathrm{H} = {\mathrm{\Sigma H}}_{\mathrm{products}} - {\mathrm{\Sigma H}}_{\mathrm{reactants}}$

• $∆\mathrm{H} = ∆\mathrm{U} + \mathrm{p}∆\mathrm{V}$

• $∆\mathrm{H}{°}_{\left(\mathrm{reaction}\right)} = \mathrm{\Sigma H}{°}_{(\mathrm{products} \mathrm{bonds})} - \mathrm{\Sigma H}{°}_{(\mathrm{reactant} \mathrm{bonds})}$

• $∆\mathrm{H} = ∆\mathrm{U} + ∆\mathrm{nRT}$

For the process A (1, 0.05 atm, 32°C) → A (g, 0.05 atm, 32°C)

The correct set of thermodynamic parameters is

• $∆$G = 0 and $∆$S = -ve

• $∆$G = 0 and $∆$S = +ve

• $∆$G = +ve and $∆$S = 0

• $∆$G = -ve and $∆$S = 0

The standard enthalpy of formation of H₂O (l) and Fe₂O₃ (s) are respectively -286 kJ mol^-1 and -824 kJ mol^-1. What is the standard enthalpy change for the following reaction?

Fe₂O₃ (s) + 3H₂ (g) → 3H₂O (l) + 2Fe (s)

• -538 kJ mol^-1

• +538 kJ mol^-1

• -34 kJ mol^-1

• +34 kJ mol^-1