Thermodynamics Questions | JEE Main Chemistry Chapter Wise Question Papers

(1)

$Option (A)$

$W = - n R T \ln \frac{V_{2}}{V_{1}}$

$= \frac{- 2 \times 8.314 \times 300}{1000} \times \ln (\frac{20}{2}) kJ$

$= - 11.5 kJ$

$Option (B)$

$W = - P_{ext} [V_{2} - V_{1}]$

$= - 3 [3 - 1]$

$= - 6 kJ$

$Option (C)$

$Δ U = n C_{v} Δ T$

$= 1 \times \frac{3}{2} \times \frac{8.314 \times 320}{1000} kJ$

$= 3.99 kJ$

$Option (D)$

$Δ H = n C_{p} Δ T$

$= 1 \times \frac{5}{2} \times \frac{8.314 \times 337}{1000} kJ$

$= 7 kJ$

(1)

${CH}_{4} (g) \to C (g) + 4 H (g); Δ_{r} H = x kJ/mol$

$C_{2} H_{6} (g) \to 2 C (g) + 6 H (g); Δ_{r} H = y kJ/mol$

$1000 x = 4 \times ε_{C - H}$

$1000 y = 1 \times ε_{C - C} + 6 \times ε_{C - H}$

$ε_{C - C} = (y - \frac{3 x}{2}) \times 1000 = \frac{h c}{λ} \cdot N_{A}$

$(λ') wavelength of photon = \frac{h c N_{A}}{[4 y - 6 x] \times 250}$

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	List-I		List-II
	Thermodynamic Process		Magnitude in kJ
A.	Work done in reversible, isothermal expansion of 2 mol of ideal gas from $2 {dm}^{3}$ to $20 {dm}^{3}$ at 300 K.	I.	4
B.	Work done in irreversible isothermal expansion of 1 mol ideal gas from $1 m^{3}$ to $3 m^{3}$ at 300 K against a constant pressure of 3 kPa.	II.	11.5
C.	Change in internal energy for adiabatic expansion of a 1 mol ideal gas with change of temperature = 320 K and ${\bar{C}}_{V} = \frac{3}{2} R$ .	III.	6
D.	Change in enthalpy at constant pressure of 1 mol ideal gas with change of temperature = 337 K and ${\bar{C}}_{P} = \frac{5}{2} R$ .	IV.	7

	Column – I		Column – II
	(Graphs)		(Area shown in the graph represents the magnitude of)
A)		P)	q
B)		Q)	w
C)		R)	$(ΔG) T$
D)		S)	$(ΔG) P$