Given, $∆$G°=-nFE°_cell and $∆$G° = -RT ln k. The value of n = 2 will be given by the slope of which line in the figure

• OA

• OB

• OC

• OD

The standard molar heat of formation of ethane, CO₂ and water (l) are respectively -21.1, -94.1 and -68.3 kcal. The standard molar heat of combustion of ethane will be

• -372 kcal

• 162 kcal

• -240 kcal

• 183.5 kcal

For the given reaction,

H₂ (g) + Cl₂ (g) → 2H⁺ (aq) + 2Cl^- (aq); $∆\mathrm{G}°$ = -262.4 kJ

The value of free energy of formation ($∆\mathrm{G}{°}_{\mathrm{f}}$) for the ion Cl^-1 (aq), therefore will be

• -131.2 kJ mol^-1

• +131.2 kJ mol^-1

• -262.4 kJ mol^-1

• +262.4 kJ mol^-1

When 1 mole of CO₂ (g) occupying volume 10 L at 27°C is expanded under adiabatic condition, temeprature falls to 150 K. Hence, final volume is

• 5 L

• 20 L

• 40 L

• 80 L

Match List I (Equations) with List II (Types of process) and select the correct option.

	List I (Equation)		List II (Types of process)
A.	${\mathrm{K}}_{\mathrm{p}} >\mathrm{Q}$	1.	Non-spontaneous
B.	$∆\mathrm{G}° < \mathrm{RT} \mathrm{in} \mathrm{Q}$	2.	Equilibrium
C.	${\mathrm{K}}_{\mathrm{p}} =\mathrm{Q}$	3.	Spontaneous and endothermic
D.	T > $\frac{∆\mathrm{H}}{∆\mathrm{S}}$	4.	Spontaneous

• A	B	C	D
  1	2	3	4

• A	B	C	D
  3	4	2	1

• A	B	C	D
  4	1	2	3

• A	B	C	D
  2	1	1	3

Consider the following processes $∆\mathrm{H} (\mathrm{kJ}/\mathrm{mol})$

      $$\begin{gathered} \frac{1}{2}\mathrm{A} \to \mathrm{B} + 150 \\ 3\mathrm{B} \to 2\mathrm{C} + \mathrm{D} - 125 \\ \mathrm{E}+\mathrm{A} \to 2\mathrm{D} + 350 \\ \mathrm{for} \mathrm{B}+ \mathrm{D} \to \mathrm{E} + 2\mathrm{C}, ∆\mathrm{H} \mathrm{will} \mathrm{be} \end{gathered}$$

• 525 k.J/mol

• -175 kJ/mol

• -325kJ/mol

• 325 kJ/mol

Heat of formation, $∆{\mathrm{H}}_{\mathrm{f}}^{°}$ of an explosive compound like NCl₃ is

• positive

• Negative

• Zero

• Positive or Negative

For the reaction,

$$\begin{gathered} {\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right) + 5{\mathrm{O}}_2\left(\mathrm{g}\right) \to 3{\mathrm{CO}}_2\left(\mathrm{g}\right) + 4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) \mathrm{at} \mathrm{constant} \mathrm{temperature}, \\ ∆\mathrm{H}-∆\mathrm{E} \mathrm{is} \end{gathered}$$

• RT

• -3RT

• 3RT

• -RT

359.

The favourable conditions for a spontaneous reaction are

• $\mathrm{T} ∆\mathrm{S} >∆\mathrm{H}, ∆\mathrm{H}=+\mathrm{ve}, ∆\mathrm{S}= +\mathrm{ve}$

• $\mathrm{T} ∆\mathrm{S} >∆\mathrm{H}, ∆\mathrm{H}=+\mathrm{ve}, ∆\mathrm{S}= -\mathrm{ve}$

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

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

Enthalpy of a compound is equal to its

• heat of combustion

• heat of formation

• heat of reaction

• heat of solution