Please be patient as the PDF generation may take upto a minute.

A 10 g piece of iron (C = 0.45 J/g°C) at 100 °C is dropped into 25 g of water (C = 4.2 J/g°C) at 27°C. Find the temperature of the iron and water system at thermal equilibrium.
1. 30 °C
2. 33 °C
3. 40 °C
4. None of these

2 mole of zinc is dissolved at HCI at $25°\mathrm{C}$.
The work done in open vessel is:
1. -2.477 KJ
2. -4.955 KJ
3. 0.0489 KJ
4. None

A sample of an ideal gas is expanded 1 ${\mathrm{m}}^3$ to 3 ${\mathrm{m}}^3$ in a reversible process for which P = K${\mathrm{V}}^2$, with K = 6 bar/m. Work done by the gas is
1. 5200 kJ
2. 15600 kJ
3. 52 kJ
4. 5267.6 kJ

An ideal gas is taken around the cycle ABCA as shown in P-V diagram. The network done during the cycle is equal to :
                            
1. 12 ${\mathrm{P}}_1{\mathrm{V}}_1$
2. 6 ${\mathrm{P}}_1{\mathrm{V}}_1$
3. 5 ${\mathrm{P}}_1{\mathrm{V}}_1$
4. ${\mathrm{P}}_1{\mathrm{V}}_1$

A gas expands against a variable pressure given by P = 20/V (where P in atm and V in L). During expansion from the volume of 1 liter to 10 liters, the gas undergoes a change in internal energy of 400 J. How much heat is absorbed by the gas during expansion?
1. 46 J
2. 4660 J
3. 5065.8 J
4. 4260 J

5 mole of an ideal gas expand isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 1 atm, ${\mathrm{W}}_{\mathrm{irr}}$ at 300 K is:
1. -15.921 KJ
2. -11.224 KJ
3. -110.83 KL
4. None of these

One mole of a non-ideal gas undergoes a change of state from (1.0 atm, 3.0 L, 200 K) to (4.0 atm, 5.0 L, 250 K) with a change in internal energy ($∆$U) = 40 L-atm. The change in enthalpy of the process in L-atm:
1. 43
2. 57
3. 42
4. None of these

Consider the reaction at 300 K ${\mathrm{C}}_6{\mathrm{H}}_6\left(\mathrm{l}\right) + \frac{15}{2}{\mathrm{O}}_2\left(\mathrm{g}\right) \to 6{\mathrm{CO}}_2\left(\mathrm{g}\right) +3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{I}\right); (∆\mathrm{H}) = -3271 \mathrm{kJ}$. What is AU for the combustion of 1.5 moles of benzene at 27°C
1. -3267.25 kJ
2. -4900.88 kJ
3. -4906.5 kJ
4. -3274.75 kJ

When two moles of an ideal gas (${\mathrm{C}}_{\mathrm{P}, \mathrm{m}}$ = $\frac{5}{2}$R) heated from 300 K to 600 K at constant pressure. The change in entropy of gas $∆$S is
1. $\frac{3}{2} \mathrm{R} \mathrm{In} 2$
2. - $\frac{3}{2} \mathrm{R} \mathrm{In} 2$
3. $5 \mathrm{R} \mathrm{In} 2$
4. $\frac{5}{2} \mathrm{R} \mathrm{In} 2$

When one mole of an ideal gas is compressed to half of its initial volume and simultaneously heated to twice its initial temperature, the change in entropy of gas ($∆$S) is :
1. ${\mathrm{C}}_{\mathrm{P}, \mathrm{m}}$ In 2
2. ${\mathrm{C}}_{\mathrm{v}, \mathrm{m}}$ In 2
3. R In 2
4. (${\mathrm{C}}_{\mathrm{v}, \mathrm{m}}$ = R) In 2

What is the change in entropy when 2.5 moles of water is heated from 27 °C to 87°C? Assume that the capacity is constant (${\mathrm{C}}_{\mathrm{P},\mathrm{m}} \left({\mathrm{H}}_2\mathrm{O}\right) = 4.2 \mathrm{J}/\mathrm{g}-\mathrm{k} \mathrm{in} \left(1.2\right) = 0.18$)
1. 16.6 J/K
2. 9 J/K
3. 34.02 J/K
4. 1.89 J/K

At 25 °C, $∆\mathrm{G}°$ for the process ${\mathrm{H}}_2\mathrm{O}$(l) $\rightleftharpoons$ ${\mathrm{H}}_2\mathrm{O}$(g) is 8.6 kJ. The vapor pressure of water at this temperature is near:
1. 24 torr
2. 285 torr
3. 32.17 torr
4. 100 torr

The standard enthalpy of formation of gaseous ${\mathrm{H}}_2\mathrm{O}$ at 298 K is -241.82 kJ/mol. Calculate $∆\mathrm{H}°$ at 373 K given the following values of the molar heat capacities at constant pressure:
${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) = 33.58 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-4}$; ${\mathrm{H}}_2\left(\mathrm{g}\right) = 29.84 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$; ${\mathrm{O}}_2\left(\mathrm{g}\right) = 29.37 {\mathrm{JK}}^{-1} {\mathrm{mol}}^{-1}$.
Assume that the heat capacities are independent of temperature :
1. -242.6 kJ/mol
2. -485.2 kJ/mol
3. -121.3 kJ/mol
4. -286.4 kJ/mol

Gasoline has an enthalpy of combustion 24000 kJ/gallon. When gasoline burns in an automobile engine, approximately 30% of the energy released is used to produce mechanical work. The remainder is lost as heat transfer to the engine's cooling system. As a start on estimating how much heat transfer is required, calculate what mass of water could be heated from 25 °C to 75 °C by the combustion of 1.0 gallons of gasoline in an automobile? (Given : C(${\mathrm{H}}_2\mathrm{O}$) = 4.18 J/g°C)
1. 34.45 kg
2. 80.383 kg
3. 22 kg
4. 224 kg

A 0.05 L sample of 0.2 M aqueous hydrochloric acid is added to 0.05 L of 0.2 M aqueous ammonia in a calorimeter. The heat capacity of the entire calorimeter system is 480 J/K. The temperature increase is 1.09 K. Calculate $∆\mathrm{rH}°$ in kJ/mol for the following reaction:
$\mathrm{HCl}(\mathrm{aq}.)+{\mathrm{NH}}_3\left(\mathrm{aq}\right) \to {\mathrm{NH}}_4\mathrm{Cl}(\mathrm{aq}.)$
1. -52.32
2. -61.1
3. -55.8
4. -58.2

Boron can undergo the following reactions with the given enthalpy changes: 2B(s)
$2\mathrm{B}\left(\mathrm{s}\right) + \frac{3}{2}{\mathrm{O}}_2 \to {\mathrm{B}}_2{\mathrm{O}}_2\left(\mathrm{s}\right); ∆\mathrm{H} = -1260 \mathrm{kJ}$
$2\mathrm{B}\left(\mathrm{s}\right) + 3{\mathrm{H}}_2 \to {\mathrm{B}}_2{\mathrm{H}}_6\left(\mathrm{s}\right); ∆\mathrm{H} = 30 \mathrm{kJ}$
Assume no other reactions are occurring. If in a container (operating at constant pressure) which is isolated from the surrounding, a mixture of H2(gas) and ${\mathrm{O}}_2$ (gas) is passed over excess of B(s), then calculate the molar ratio (${\mathrm{O}}_2;{\mathrm{H}}_2$) so that the temperature of the container does not change :
1. 15:3
2. 42:1
3. 1:42
4. 1:84