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A heating coil is immersed in a 100 g sample of ${\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$ at 1 atm and 100$°$C in a closed vessel. In this heating process, 60% of the liquid is converted in to gaseous form at constant pressure of 1 atm. Densities of liquid and gaseous water under these conditions are 1000 kg/m³ and 0.60 kg/m³ respectively. Magnitude of the work done for the process is:
1.  4997 J
2.  4970 J
3.  9994 J
4.  None of these

What is the value of change in internal energy at 1 atm in the process?
                                   ${\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}, 323 \mathrm{K}\right) \to {\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}, 423 \mathrm{K}\right)$
Given: ${\mathrm{C}}_{\mathrm{v}, \mathrm{m}} \left({\mathrm{H}}_2\mathrm{O}, \mathrm{l}\right)=75.0 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1} ; {\mathrm{C}}_{\mathrm{p}, \mathrm{m}} \left({\mathrm{H}}_2\mathrm{O}, \mathrm{g}\right)=33.314 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$
            $△{\mathrm{H}}_{\mathrm{vap}} \mathrm{at} 373 \mathrm{K}=40.7 \mathrm{kJ}/\mathrm{mol}$
1.  42.91 kJ/mol
2.  43086 kJ/mol
3.  42.6 kJ/mol
4.  49.6 kJ/mol

A gas $\left({\mathrm{C}}_{\mathrm{v}, \mathrm{m}}=\frac{5}{2}\mathrm{R}\right)$ behaving ideally was allowed to expand reversibly and adiabatically from 1 litre to 32 litre. It's initial temperature was 327$°$C. The molar enthalpy change (in J/mol) for the process is:
1.  -1125 R
2.  -675
3.  -1575 R
4.  None of these

Two moles of an ideal gas is heated at a constant pressure of one atmosphere from 27$°$C to 127$°$C. If ${\mathrm{C}}_{\mathrm{v}, \mathrm{m}}=20+{10}^{-2} \mathrm{T} {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1},$ then q and $△\mathrm{U}$ for the process are respectively:
1.  6362.8 J, 4700 J
2.  3037.2 J, 4700 J
3.  7062.8 J, 5400 J
4.  3181.4 J, 2350 J

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

2 mole of an ideal monoatomic gas undergoes a reversible process for which PV²=C. The gas is expanded from initial volume of 1 L to final volume of 3 L starting from initial temperature of 300 K. Find $△\mathrm{H}$ for the process:
1.  -600 R
2.  -1000 R
3.  -3000 R
4.  None of these

Calculate $△\mathrm{S}$ for 3 mole of a diatomic ideal gas which is heated and compressed from 298 K and 1 bar to 596 K and 4 bar: [Given: C_{v, m} (gas)=$\frac{5}{2}$ R;  ln (2)=0.70;  R=2 cal k^-1 mol^-1]
1.  -14.7 cal K^-1
2.  +14.7 cal K^-1
3.  -6.9 cal K^-1
4.  6.3 cal K^-1

One mole of an ideal monoatomic gas at 27$°$C is  subjected to a reversible isentropic compression until final temperature reaches to 327$°$ C. If the initial pressure was 1.0 atm then find the value of (ln P₂):  (Given : ln 2 = 0.7)
1.  1.75 atm
2.  0.176 atm
3.  1.0395 atm
4.  2.0 atm

Two moles of an ideal gas is expanded irreversibly and isothermally at 37$°$C until its volume is doubled and 3.41 kJ heat is absorbed from surrounding. $△{\mathrm{S}}_{\mathrm{total}}$ (system+surrounding) is:
1.  -0.52 J/K
2.  0.52 J/K
3.  22.52 J/K
4.  0

Combustion of sucrose is used by aerobic organisms for providing energy for the life sustaining processes. If all the capturing of energy from the reaction is done through electrical process (non P-V work) then calculate maximum available energy which can be captured by combustion of 34.2 gm of sucrose
Given : $△{\mathrm{H}}_{\mathrm{combustion}} \left(\mathrm{sucrose}\right)=-6000 \mathrm{kJ} {\mathrm{mol}}^{-1}$
           $△{\mathrm{S}}_{\mathrm{combustion}} =180 \mathrm{J}/\mathrm{K}‐\mathrm{mol} \mathrm{and} \mathrm{body} \mathrm{temperature} \mathrm{is} 300 \mathrm{K}$
1.  600 kJ
2.  594.6 kJ
3.  5.4 kJ
4.  605.4 kJ

For the hypothetical reaction
                                    ${\mathrm{A}}_2\left(\mathrm{g}\right)+{\mathrm{B}}_2\left(\mathrm{g}\right) \rightleftharpoons 2\mathrm{AB}\left(\mathrm{g}\right)$
${△}_{\mathrm{r}}{\mathrm{G}}^{\circ } \mathrm{and} {△}_{\mathrm{r}}{\mathrm{S}}^{\circ }$ are 20 kJ/mol and -20 JK^-1 mol^-1 respectively at 200 K.
If ${△}_{\mathrm{r}}{\mathrm{C}}_{\mathrm{P}}$ is 20 JK^-1 mol^-1 then ${△}_{\mathrm{r}}{\mathrm{H}}^{\circ }$ at 400 K is:
1.  20 kJ/mol
2.  7.98 kJ/mol
3.  28 kJ/mol
4.  None of these

Calculate ${△}_{\mathrm{f}}{\mathrm{G}}^{\circ }$ for $\left({\mathrm{NH}}_4\mathrm{Cl}, \mathrm{s}\right)$ at 310 K.
Given : ${△}_{\mathrm{f}}{\mathrm{H}}^{\circ } \left({\mathrm{NH}}_4\mathrm{Cl}, \mathrm{s}\right)=-314 \mathrm{kJ}/\mathrm{mol}; {△}_{\mathrm{r}}{\mathrm{C}}_{\mathrm{p}}=0$
${\mathrm{S}}^{\circ }{\mathrm{N}}_2 \left(\mathrm{g}\right)=192 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}; {\mathrm{S}}^{\circ }{\mathrm{H}}_2 \left(\mathrm{g}\right)=130.5 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1};$
${\mathrm{S}}^{\circ }{\mathrm{Cl}}_2 \left(\mathrm{g}\right)=233 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}; {\mathrm{S}}^{\circ }{\mathrm{NH}}_4\mathrm{Cl} \left(\mathrm{s}\right)=99.5 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$
All given data at 300 K.
1.  –198.56 kJ/mol
2.  –426.7 kJ/mol
3.  –202.3 kJ/mol
4.  None of these

Fixed mass of an ideal gas contained in a 24.63 L sealed rigid vessel at 1 atm is heated from -73$°$C to 27$°$.Calculate change in Gibb's energy if entropy of gas is a function of temperature as S=2+10^-2 T(J/K): (Use 1 atm L=0.1 kJ)
1.  1231.5 J
2.  1281.5 J
3.  781.5 J
4.  0

The molar heat capacities at constant pressure (assumed constant with respect to temperature) of A, B and C are in ratio of 3 : 1.5 : 2.0. The enthalpy change for the exothermic reaction A+2B $\to$ 3C at 300 K and 310 K is $△{\mathrm{H}}_{300} \mathrm{and} △{\mathrm{H}}_{310}$ respectively then:
1.  $△{\mathrm{H}}_{300} > △{\mathrm{H}}_{310}$
2.  $△{\mathrm{H}}_{300} < △{\mathrm{H}}_{310}$
3.  $△{\mathrm{H}}_{300} = △{\mathrm{H}}_{310}$
4.  $\mathrm{if} {\mathrm{T}}_2>{\mathrm{T}}_1 \mathrm{then} △{\mathrm{H}}_{310} > △{\mathrm{H}}_{300} \mathrm{and} \mathrm{if} {\mathrm{T}}_2<{\mathrm{T}}_1 \mathrm{then} △{\mathrm{H}}_{310} < △{\mathrm{H}}_{300}$

Determine $△{\mathrm{U}}^{\circ }$ at 300 K for the following reaction using the listed enthalpies of reaction:
$\begin{array}{ccc}4\mathrm{CO}\left(\mathrm{g}\right)+8{\mathrm{H}}_2\left(\mathrm{g}\right)& \to & 3{\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\\ \mathrm{C}\left(\mathrm{graphite}\right)+1/2 {\mathrm{O}}_2 \left(\mathrm{g}\right)& \to & \mathrm{CO}\left(\mathrm{g}\right); △{{\mathrm{H}}_1}^{\circ }=-110.5 \mathrm{kJ}\\ \mathrm{CO}\left(\mathrm{g}\right)+1/2 {\mathrm{O}}_2 \left(\mathrm{g}\right)& \to & {\mathrm{CO}}_2\left(\mathrm{g}\right); △{{\mathrm{H}}_2}^{\circ }=-282.9 \mathrm{kJ}\\ {\mathrm{H}}_2\left(\mathrm{g}\right)+1/2 {\mathrm{O}}_2 \left(\mathrm{g}\right)& \to & {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); △{{\mathrm{H}}_3}^{\circ }=-285.8 \mathrm{kJ}\\ \mathrm{C}\left(\mathrm{graphite}\right)+2{\mathrm{H}}_2 \left(\mathrm{g}\right)& \to & {\mathrm{CH}}_4\left(\mathrm{g}\right); △{{\mathrm{H}}_4}^{\circ }=-74.8 \mathrm{kJ}\end{array}$
1.  -653.5 kJ
2.  -686.2 kJ
3.  -747.4 kJ
4.  None of these

Calculate ${△}_{\mathrm{f}}\mathrm{H}°$ (in kJ/mol) for ${\mathrm{Cr}}_2{\mathrm{O}}_3$ from the ${△}_{\mathrm{r}}\mathrm{G}°$ and the $\mathrm{S}°$ values provided at 27$°$C
$4\mathrm{Cr}\left(\mathrm{s}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)$ $\to$ $2{\mathrm{Cr}}_2{\mathrm{O}}_3\left(\mathrm{s}\right);$ $$
${△}_{\mathrm{r}}\mathrm{G}°=-2093.4$ $\mathrm{kJ}/\mathrm{mol}$
$\mathrm{S}°\left(\mathrm{J}/\mathrm{K}\right)$ $\mathrm{mol}$ $:$ $\mathrm{S}°\left(\mathrm{Cr},\right)$ $\mathrm{s}=24;$ $$
$\mathrm{S}°\left({\mathrm{O}}_2,\right)$ $\mathrm{g}=205;$ $$ $$ $\mathrm{S}°\left({\mathrm{Cr}}_2{\mathrm{O}}_3,\right)$ $\mathrm{s}=81$
1.  -2258.1 kJ/mol
2.  -1129.05 kJ/mol
3.  -964.35 kJ/mol
4.  None of the above

When 1.0 g of oxalic acid $\left({\mathrm{H}}_2{\mathrm{C}}_2{\mathrm{O}}_4\right)$ is burned in a bomb calorimeter whose heat capacity is 8.75 kJ/K, the temperature increases by 0.312 K. The enthalpy of combustion of oxalic acid at 27$°$C is:
1.  -245.7 kJ/mol
2.  -244.452 kJ/mol
3.  -246.947 kJ/mol
4.  None of these

The enthalpy of neutralization of a weak monoprotic acid (HA) in 1 M solution with a strong base is -55.95 kJ/mol. If the unionized acid is required 1.4 kJ/mol heat for it's complete ionization and enthalpy of neutralization of the strong monobasic acid with a strong monoacidic base is -57.3 kJ/mol. What is the % ionization of the weak acid in molar solution?
1.  1%
2.  3.57%
3.  35.7%
4.  10%

Determine C$-$C and C$-$H bond enthalpy (in kJ/mol)
$\mathrm{Given} : {△}_{\mathrm{f}}\mathrm{H}°\left({\mathrm{C}}_2{\mathrm{H}}_6, \mathrm{g}\right)=-85 \mathrm{kJ}/\mathrm{mol}, {△}_{\mathrm{f}}\mathrm{H}°\left({\mathrm{C}}_3{\mathrm{H}}_8, \mathrm{g}\right)=-104 \mathrm{kJ}/\mathrm{mol}$
${△}_{\mathrm{sub}}\mathrm{H}° \left(\mathrm{C}, \mathrm{s}\right)=718\mathrm{kJ}/\mathrm{mol}, \mathrm{B}.\mathrm{E}. \left(\mathrm{H}-\mathrm{H}\right)=436 \mathrm{kJ}/\mathrm{mol}$
1.  414, 345
2.  345, 414
3.  287, 404.5
4.  None of these