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Enthalpy of neutralisation of acetic acid by NaOH is -50.6 kJ/mol and the heat of  neutralisation of strong acid with a strong base is -55.9 kJ/mol. What is the value of $∆H$ for ionisation of CH₃COOH?
(1) +5.3 kJ/mol
(2) +6.2 kJ/mol
(3) +8.2 kJ/mol
(4) +9.3 kJ/mol

The values of heat of formation of SO₂ and SO₃ are -298.2 kJ and -98.2 kJ . The heat of reaction of the following reaction will be: SO₂+$\frac{1}{2}{O}_2\to S{O}_3$
(1) -200 kJ
(2) -356.2 kJ
(3) +200 kJ
(4) -396.2 kJ

For which of the following $∆U=∆H$?
(1) N₂O_4(g) $\rightleftharpoons$2NO_2(g)
(2) 2SO_2(g) + O_2(g) $\rightleftharpoons$2SO_3(g)
(3) H_2(g) + Cl_(2)(g) $\rightleftharpoons$ 2HCl_(g)
(4)H_2(g)+$\frac{1}{2}{O}_{2\left(g\right)}$ $\rightleftharpoons$H₂O_(l)

If the heat of combustion of carbon monoxide at constant volume and at 17$°$C is -283.3 kJ then its heat of combustion at constant pressure: (R=8.314 J degree^-1 mol^-1)
(1) -284.5 kJ
(2) 284.5 kJ
(3) 384.5 kJ
(4) -384.5 kJ

The entropy change in the conversion of one mole of liquid water at 373 K to vapour at the same temperature would be: (Latent heat of vaporization of water, $∆H_{vap}=2.257$ $kJ/g$)
1. 105.9 JK^-1mol^-1
2. 107.9 JK^-1mol^-1
3. 108.9 JK^-1mol^-1
4. 109.9 JK^-1mol^-1

The molar heat capacity of water at constant pressure is 75 JK^-1 mol^-1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase is temperature of water is:
(1) 6.6 K
(2) 1.2 K
(3) 2.4 K
(4) 4.8 K

If the bond energies of H-H, Br-Br and HBr are 433, 192 and 364 kJ mol^-3 respectively the $∆H^{+}$ for the reaction, ${\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{Br}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{HBr}}_{\left(\mathrm{g}\right)}$ is:
(1) +261 kJ
(2) -103 kJ
(3) -261 kJ
(4) +103 kJ

The enthalpy of hydrogenation of cyclohexene is -119.5 kJ mol^-1. If resonance energy of benzene is -150.4 kJ mol^-1, its enthalpy of hydrogenation would be:
(1) -269.9 kJ mol^-1
(2) -358.5 kJ mol^-1
(3) -508.9 kJ mol^-1
(4) -208.1 kJ mol^-1

The enthalpy change $(∆H)$ for the reaction. ${\mathrm{N}}_{2\left(\mathrm{g}\right)}+3{\mathrm{H}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{NH}}_{3\left(\mathrm{g}\right)}$ is -92.38 kJ at 298 K. The internal energy change $∆U$ at 298 K is:
(1) -92.38 kJ
(2) -87.42 kJ
(3) -97.34 kJ
(4) -89.9 kJ

If w is the amount of work done by the system and q is the amount of heat supplied to the system, identify the type of the system:
(1) Isolated system
(2) Closed system
(3) Open system
(4) System with thermally conducting walls

When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0$°$C and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in kJ
$[∆{\mathrm{H}}_{\mathrm{comb}.}({\mathrm{CH}}_4)=890 \mathrm{kJ} {\mathrm{mol}}^{-1}, ∆{\mathrm{H}}_{\mathrm{comb}.}({\mathrm{CH}}_3{\mathrm{H}}_8)=2220 \mathrm{kJ} {\mathrm{mol}}^{-1}]$ is:
(1) 38
(2) 317
(3) 477
(4) 32

10 mole of an ideal gas is heated at constant pressure of one atmosphere from $27°\mathrm{C} \mathrm{to} 127°\mathrm{C}$. If ${\mathrm{C}}_{\mathrm{v},\mathrm{m}}=21.686+{10}^{-3} \mathrm{T}\left({\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}\right), \mathrm{then} ∆\mathrm{H}$ for the process is:
(1) 3000 J
(2) 3350 J
(3) 3700 J
(4) 30350 J

For polytropic process ${\mathrm{PV}}^{\mathrm{n}}$=constant, molar heat capacity $\left({\mathrm{C}}_{\mathrm{m}}\right)$ of an ideal gas is given by:
(1) ${\mathrm{C}}_{\mathrm{v},\mathrm{m}}+\frac{\mathrm{R}}{(\mathrm{n}-1)}$
(2) ${\mathrm{C}}_{\mathrm{v},\mathrm{m}}+\frac{\mathrm{R}}{(1-\mathrm{n})}$
(3) ${\mathrm{C}}_{\mathrm{v},\mathrm{m}}+\mathrm{R}$
(4) ${\mathrm{C}}_{\mathrm{p},\mathrm{m}}+\frac{\mathrm{R}}{(\mathrm{n}-1)}$

One mole of an ideal monoatomic gas at $27°\mathrm{C}$ is subjected to a reversible isoentropic compression until final temperature reaches to $327°C$. If the initial pressure was 1.0 atm then find the value of $(\ln {\mathrm{P}}_2):(\mathrm{Given}:\ln 2=0.7)$
(1) 1.75 atm
(2) 0.176 atm
(3) 1.0395 atm
(4) 2.0 atm