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Molar and Spe...

Molar and Specific Heat Capacity

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Q.

In a constant volume calorimeter, $3.5 g$ of a gas with molecular weight 28 was burnt in excess of oxygen at $298 k$ . The temperature of the calorimeter was found to Increase from $298 k$ to $298.45 k$ due to the combustion process. Given that the heat capacity of the calorimeter is $2.5 K J / K$ . The Numerical value for the enthalpy of combustion of the Gas in KJ /Mole is

10.8
20
25
9

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Q.

Match the $\frac{C_{p}}{C_{v}}$ ratio for ideal gases with the different types of molecules:

Column 1	Column 2
Monoatomic	$\frac{7}{5}$
Diatomic rigid molecules	$\frac{9}{7}$
Diatomic non rigid molecules	$\frac{4}{3}$
Triatomic rigid molecules	$\frac{5}{3}$

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Q. 30.in a thermodynamic process on an ideal diatomic gas, work done by gas is n times the heat supplied (n<1) find the molar heat capacity of gas for the process

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Q.

Calculate change in internal energy for 2 moles of an ideal gas that temperature rises from 27 $^{\circ}$ C to 127 $^{\circ}$ C. [ Given : Cp, m = 13.314 + 0.04 T ]

None of these
3800 J
1900 J
1028 J

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Q. Calculate the standard free energy change for the formation of methane at 298 K.

C_{(g r a p h i t e)} + 2 H_{2 (g)} \to C H_{4 (g)}

Given that,

Δ o f C H_{4} = - 74.81 K J m o l^{- 1}

and

Δ S^{\circ} o f C_{g r a p h i t e}, H_{2 (g)} a n d C H_{4 (g)} a r e 5.70 K^{- 1} m o l^{- 1}, a n d 186.3 J K^{- 1} m o l^{- 1}

respectively.

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Q. If ∆q amount of heat energy is provided to a monoatomic gas sample having two moles in a process PT=constant then increase in temperature of gas is equal to

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Q.

The sulphur dioxide obtained by the combustion of 8 g of sulphur is passed into Bromine water. The solution is then treated with barium chloride solution. The amount of barium sulphate formed is

1 mole
0.5 mole
0.25 g
0.25 gm moles

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Q. ratio of molar heat capacity at cons†an t volume to its specific heat capacity at cons†an t voulme for hydrogen is equal t

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Q. The molar specific heat of hydrogen at constant volume is

5 c a l / m o l^{o} C

. Heat required to raise the temperature of 1 gm

H_{2}

gas by

10^{o} C

at constant volume is

22 cal
40 cal
20 cal
25 cal

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Q. Enthalpy of combustion of carbon to

C O_{2}

is -393.5 kJ

m o l^{- 1}

. Calculate the heat released upon formation of 35.2g of

C O_{2}

from carbon and dioxygen gas.

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Q. Ice-water mass ratio is maintained as 1 : 1 in a given system containing water in equilibrium with ice at constant pressure. If

C_{P} (i c e) = C_{P} (w a t e r) = 4.18 J g^{- 1} K^{- 1}

then molar heat capacity of such a system is

Zero
Infinity
$4.182 J K^{- 1} m o l^{- 1}$
$75.48 J K^{- 1} m o l^{- 1}$

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Q. Ice-water mass ratio is maintained as 1 : 1 in a given system containing water in equilibrium with ice at constant pressure. If

C_{P} (i c e) = C_{P} (w a t e r) = 4.18 J g^{- 1} K^{- 1}

then molar heat capacity of such a system is

Zero
Infinity
$4.182 J K^{- 1} m o l^{- 1}$
$75.48 J K^{- 1} m o l^{- 1}$

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Q.

For an ideal gas $(\frac{C_{P}}{C_{v}} = γ)$ ; of molar mass M, its specific heat capacity at constant volume is:

$\frac{γ R}{(γ - 1) M}$
$\frac{γ}{M (γ - 1)}$
$\frac{M}{R (γ - 1)}$
$\frac{γ R M}{(γ - 1)}$

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Q. Two moles of an ideal gas is heated at constant pressure of one atomsphere from

27^{\circ} C

to

127^{\circ} C .

if

C_{v, m} = 20 + 10^{- 2} T

J K^{- 1} m o l^{- 1}

then Heat (q) and Internal energy (

△ U

) for the process are respectively:

6362.8 J, 4700 J
3037.2 J, 4700 J
7062.8 J, 5400 J
3181.4 J, 2350 J

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Q. When 20 cal of heat is supplied to a system, the increase in internal energy is 50 J. If the external work done is 35 J, the mechanical equivalent of heat is:

4.92 J/cal
2.1 J/cal
4.25 J/cal
1.26 J/cal

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Q. A diatomic ideal gas initially at

273 K

is given

100 c a l

heat due to which system did

209 J

work. Molar heat capacity

(C_{m})

of gas for the process is:

$\frac{3}{2} R$
$\frac{5}{2} R$
$\frac{5}{4} R$
$5 R$

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Q. Consider the following reactions at

10000^{\circ} C

.

(a) Z n (s) + \frac{1}{2} O_{2} (g) \to Z n O (s); Δ G^{\circ} = - 360 k J / m o l (b) C (s) + \frac{1}{2} O_{2} (g) \to C O (s); Δ G^{\circ} = - 460 k J / m o l

Then choose the correct statement from the following.

Zinc can be oxidised by $C O$
$Z n O$ can be reduced by $C$
$Z n O$ can be reduced by $C O$
None of the above

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Q. Consider a system containing one mole of a diatomic gas, contained by a piston. What is the temperature change of the gas, if

q = 50 J

and

W = - 100 J ?

(Given

C_{v} = \frac{5}{2} R

)

$- 50 K$
$- 2.4 K$
$- 5.8 K$
$- 1.25 K$

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Q. 1 mole of

N H_{3}

gas at

27^{\circ} C

is expanded under adiabatic condition to make volume 8 times

(υ = 1.33)

. Final temperature and work done, respectively are:

$150 K, 900 c a l$
$250 K, 1000 c a l$
$150 K, 400 c a l$
$200 K, 800 c a l$

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Q.

Δ U^{o}

of combustion of methane is

- X k J m o l e^{- 1}

. The value of

Δ H^{o}

is:

= $Δ U^{0}$
< $Δ U^{0}$
> $Δ U^{0}$
$= 0$

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Q. The molar heat capacity (

C_{p}

) of water at constant pressure is 75

J K^{- 1} m o l e^{- 1}

. The increase in temperature (in K) of 100 g of water when 2kJ of heat is supplied to it is:

2.4 K
3.6 K
4.8 K
5.2 K

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Q. A gas expands from a volume of 3.0

d m^{3}

to 5

d m^{3}

against a constant pressure of 3.0 atm. The work done during expansion is used to heat 10.0 mole of water of temperature 290.0 K. Calculate the final temperature of water. (Specific heat of water = 4.184

J K^{- 1} g^{- 1}

289.193 K
290.807 K
304.526 K
275.470 K

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Q.

For an ideal gas $(\frac{C_{P}}{C_{v}} = γ)$ ; of molar mass M, its specific heat capacity at constant volume is:

$\frac{γ R}{(γ - 1) M}$
$\frac{γ}{M (γ - 1)}$
$\frac{M}{R (γ - 1)}$
$\frac{γ R M}{(γ - 1)}$

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Q. Calculate

w

and

Δ U

for the conversion of

0.5

mole of water at

100^{o} C

to steak at

1

atm pressure. Heat of vaporisation of water at

100^{o} C

is

40670 J {m o l}^{- 1}

.

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Q. What is the exact difference between heat, energy, temperature and work?

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