Given that,

C (s) + O₂ (g) → CO₂ (g) ; $∆\mathrm{H}°$ = -x kJ mol^-1

2CO (g) + O₂ (g) → 2CO₂ (g) ; $∆\mathrm{H}°$ = -y kJ mol^-1

The enthalpy of formation of CO will be

• $\frac{\mathrm{y} - 2\mathrm{x}}{3}$

• $\frac{\mathrm{y} - 2\mathrm{x}}{2}$

• $\frac{2\mathrm{x} - \mathrm{y}}{2}$

• $\frac{\mathrm{x} - \mathrm{y}}{2}$

Which of the following relation is correct?

• $∆\mathrm{H} = ∆\mathrm{G} + \mathrm{T}∆\mathrm{S}$

• $∆\mathrm{H} = -∆\mathrm{G} - \mathrm{T}∆\mathrm{S}$

• $∆\mathrm{H} = ∆\mathrm{G} - \mathrm{T}∆\mathrm{S}$

• $∆\mathrm{H} = -∆\mathrm{G} + \mathrm{T}∆\mathrm{S}$

143.

If -239,- 116 and -286 kJ mol^-1 respectively. The enthalpy change for the oxidation of methanol to formaldehyde and water in kJ is

• - 136

• - 173

• 163

• -163

For an endothermic reaction where ΔH represents the enthalpy of the reaction in kJ/mol, the minimum value for the energy of activation will be

• less than ΔH 

• Zero

• more than ΔH 

• equal to ΔH 

Which of the following does not result in an increase in entropy?

• Crystallisation of sucrose form a solution

• Rusting of iron

• Conversion of ice ofwater

• Vaporisation of camphor

In an adiabatic process which of the following is true?

• q = +W

• q = 0

• $∆$E = q

• p$∆$V = 0

Equation log $\frac{{\mathrm{K}}_2}{{\mathrm{K}}_1} = \frac{∆\mathrm{H}}{2.303 \mathrm{R}} \left(\frac{{\mathrm{T}}_2 -{\mathrm{T}}_1}{{\mathrm{T}}_1 . {\mathrm{T}}_2}\right)$, n is

• van der Waals' equation

• Kirchoffs equation

• Gas equation

• van't Hoff equation

Which of the following is true for a reaction in which all the products are liquid?

• $∆\mathrm{H} = ∆\mathrm{E}$

• $∆\mathrm{H} = ∆\mathrm{W}$

• $∆\mathrm{H} > ∆\mathrm{E}$

• None of these

Cell reaction is spontaneous when

• $∆\mathrm{G}°$ is negative

• $∆\mathrm{G}°$ is positive

• $∆{\mathrm{E}}_{\mathrm{red}}^{°}$ is positive

• $∆{\mathrm{E}}_{\mathrm{red}}^{°}$ is negative

At 27°C latent heat of fusion of a compound is 2930 J/ mol, then entropy change is

• 9.77 J/mol-K

• 10.77 J/ mol-K

• 9.07 J/ mol-K

• 0.977 J/ mol-K