For which reaction will $∆$H - $∆$E = 0 ? Assume that each reaction is carried out in an open container .

• 2CO₂ (g) + O₂ (g) $\to$ 2CO₂ (g)

• PCl₅ (g) $\to$ PCl₃ (g) + Cl₂ (g)

• H₂ (g) + Br₂ (g) $\to$ 2HBr (g)

• C (s) + 2H₂O (g) $\to$ 2H₂ (g) + CO₂ (g)

82.

Match List I with List II and select the correct answer using the codes given below the lists:

List I	List II
A. $(\frac{\mathrm{\delta G}}{\mathrm{\delta P}}{)}_{\mathrm{T}}$	1.  ${\mathrm{\mu }}_{\mathrm{\pi }}$
B. $(\frac{\mathrm{\delta G}}{\mathrm{\delta T}}{)}_{\mathrm{P}}$	2.  T
C. $(\frac{\mathrm{\delta H}}{\mathrm{\delta S}}{)}_{\mathrm{P}}$	3. -S
D. $(\frac{\mathrm{\delta T}}{\mathrm{\delta P}}{)}_{\mathrm{H}}$	4. P
	5. V

• A-5, B-1, C-2, D-4

• A-5, B-3, C-2, D-4

• A-3, B-5, C-2, D-1

• A-5, B-3, C-2, D-1

For adiabatic process, which is correct?

• $∆$T = 0

• $∆$S = 0

• q = 0

• q_p = 0

Which of the following is not a thermodynamic function?

• Internal energy

• Work done

• Enthalpy

• Entropy

Which ofthe following is an intensive property ?

• Temperature

• Viscosity

• Surface tension

• All of these

Which of the following is intensive property?

• Enthalpy

• Entropy

• Specific heat

• Volume

Entropy of the universe is :

• constant

• zero

• continuously decreasing

• continuously increasing

Assertion : A reaction is spontaneous if E_cell = +ve.

Reason : For E_cell = +ve, $∆$G is always -ve.

• If both assertion and reason are true and reason is the correct explanation of assertion

• If both assertion and reason are true but reason is not the correct explanation of assertion

• If assertion is true but reason is false

• If both assertion and reason are false

Assertion : Entropy is always constant for a closed system.

Reason : Closed system is always reversible.

• If both assertion and reason are true and reason is the correct explanation of assertion

• If both assertion and reason are true but reason is not the correct explanation of assertion

• If assertion is true but reason is false

• If both assertion and reason are false.

The relation between $∆$H and $∆$E is :

• $∆$E = $\mathrm{∆}$H + nRT

• $∆$H = $∆$E - $∆$nRT

• $∆$H = $∆$E + $∆$nRT

• $∆$E = $∆$H + nRT