Thermodynamics Test

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Thermodynamics Test - 16

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Weekly Quiz Competition

Question 1
1 / -0

The specific heat capacity of water is:

A
$$1\ cal\ g^{-1}$$

B
$$10\ cal\ g^{-1}$$

C
$$2\ cal\ g^{-1}$$

D
$$30\ cal\ g^{-1}$$

Solution

The specific heat capacity of water is $$1$$ calorie g$$^{-1} \ ^oC ^{-1}$$ or $$4.186$$ joule $$g$$$$^{-1} \ ^oC ^{-1}$$.
It means to increase the temperature of $$1$$ g of water by $$1$$ deg $$C$$, the heat required is $$1$$ calorie or $$4.186$$ J.
Question 2
1 / -0

Which of the following sets represent the normal physical states of the elements concerned at $$25^{\circ}C$$ and one bar pressure, with $$\Delta H^\circ$$ (formation)$$=0$$

A
$$C(diamond), S_8(s), Na(s)$$

B
$$C(diamond)), C(graphite), Br_2(I)
$$

C
$$C(graphite), Br_2(g), P_4(white)$$

D
$$C(graphite), Br_2(I), I_2(s)
$$

Solution

$$\Delta_f H^{\circ}=0$$
$$\displaystyle C_{graphite}$$ has $$\Delta_f H^{\circ}=0$$ not diamond because it is more stable than diamond
$$Br_2$$ ; standard physical state in liquid
$$I_2 \rightarrow solid$$
Question 3
1 / -0

Which of the following are not state functions?
(I) $$q+w$$
(II) $$q$$
(III) $$w$$
(IV) $$H-TS$$

A
$$(I), (II)$$ and $$(III)$$

B
$$(II)$$ and $$(III)$$

C
$$(I)$$ and $$(IV)$$

D
$$(II), (III)$$ and $$(IV)$$

Solution

State functions or state variables depend only on the state of the system.
Here '$$w$$' represents work done and '$$q$$' represents the amount of heat so both of these are not state functions.
Question 4
1 / -0

$$n \ moles$$ of gas an ideal monatomic gas is confined in a cylinder A of volume $$V_{0}$$, pressure $$P_{0}$$ and temperature $$T_{0}$$, this cylinder is connected to another cylinder B with the help of tube of a negligible volume. The cylinder B is fitted with a movable piston which can be adjusted from outside. Initially, the piston is adjusted so that volume of B is 7$$V_{0}$$ and B is evacuated and then stopcork is opened so that gas expands and occupies the volume $$8V_{0}$$. [System is thermally isolated from the surroundings].

During this free expansion, the internal energy of the system

A
Increases

B
Decreases

C
Remains constant

D
Nothing can be said

Solution

Temperature will be unchanged during the free expansion. As the internal energy is only depend on the temperature of the system. So the internal energy will remain constant.
Ans:(C)
Question 5
1 / -0

A sample of oxygen gas expands its volume from $$3\ L\ to\ 5\ L$$ against a constant pressure of $$3\ atm$$. If work done during expansion is used to heat 10 mole of water initially present at $$290\ K$$, its final temperature will be (specific heat capacity of water = 4.18 J/kg):

A
$$292.0\ K$$

B
$$298.0\ K$$

C
$$290.8\ K$$

D
$$293.7\ K$$

Solution

Work done during expansion is equal to the heat supplied to water to raise the temperature.
$$ P({V}_{2} - {V}_{1}) = mS\Delta T$$
$$3\times 2\times 101.3 = 180\times 4.18 ( {T}_{f} - 290)$$
$$ {T}_{f} = 290.8 K$$
Question 6
1 / -0

Water of mass $$m_2$$ = 1 kg is contained in a copper calorimeter of mass $$m_1$$ = 1 kg. Their common temperature t = $$10^{0}C$$. Now a piece of ice of mass $$m_3$$ = 2 kg and temperature is $$-11^{0}C$$ dropped into the calorimeter. Neglecting any heat loss, the final temperature of system is. [specific heat of copper = 0.1 Kcal/ kg$$^{0}C$$, specific heat of water = 1 Kcal/kg$$^{0}C$$, specific heat of ice = 0.5 Kcal/kg$$^{0}C$$, latent heat of fusion of ice = 78.7 Kcal/kg]

A
$$0^{0}C$$

B
$$4^{0}C$$

C
$$- 4^{0}C$$

D
$$- 2^{0}C$$

Solution

Loss in heat from calorimeter + water as temperture changes from $$10^{0}C$$ to 0$$^{0}C$$
$$ = m_1C_110 + m_2C_210 = $$ $$1 1 10 + 1 0.1 10 = 11 kca$$l
Gain in heat of ice as its temperature changes from $$- 11^{0}C$$ to 0$$^{0}C$$$ kcal$
Hence ice and water will coexist at 0$$^{0}C$$ without any phase change
Question 7
1 / -0

Specific heat of a gas undergoing adiabatic change is

A
1

B
0

C
4

D
6

Solution

During adiabatic process, no heat is supplied to system. The term $$\partial H$$ is zero.Hence the specific heat $$\displaystyle \left ( \frac{\partial H}{\partial T} \right )$$ is zero.
Question 8
1 / -0

A liquid boils at such a temperature at which the saturated vapour pressure, as compared to atmospheric pressure, is

A
one-third

B
equal

C
half

D
double

Solution

The vapor pressure at which a liquid boils is equal to the atmospheric pressure.
Question 9
1 / -0

Specific heat may be defined as:

A
heat capacity at constant volume

B
heat capacity at constant pressure

C
heat capacity mol$$^{-1}$$

D
heat capacity g$$^{-1}$$

Solution

The amount of heat required to raise the temperature of a unit mass of a substance by one-degree celsius is known as specific heat. Heat capacity is the amount of heat added to a substance to raise its temperature by one kelvin.

Thus, specific heat may be defined as heat capacity per gram.
Question 10
1 / -0

The temperature at which the reaction $$AgO(s) \rightarrow Ag(s) + \frac{1}{2} O_2(g)$$ is at equilibrium is?
Given $$\Delta H = 30.5 KJ mol^{-1}$$ and $$\Delta S = 0.066 KJK^{-1} mol^{-1}$$

A
462.12 K

B
362.12 k

C
262.12 k

D
562.12 k

Solution

The temperature at which the reaction is at equilibrium is $$T=\frac {\Delta H}{Delta S}$$.
Substitute values in the above expression.
$$T= \frac {\Delta H = 30.5 KJ mol^{-1}} {\Delta S = 0.066 KJK^{-1} mol^{-1}}=462.12K$$

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Thermodynamics Test - 16

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Thermodynamics Test - 16

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Question 1

$$1\ cal\ g^{-1}$$

$$10\ cal\ g^{-1}$$

$$2\ cal\ g^{-1}$$

$$30\ cal\ g^{-1}$$

Solution

Question 2

$$C(diamond), S_8(s), Na(s)$$

$$C(diamond)), C(graphite), Br_2(I)$$

$$C(graphite), Br_2(g), P_4(white)$$

$$C(graphite), Br_2(I), I_2(s)$$

Solution

Question 3

$$(I), (II)$$ and $$(III)$$

$$(II)$$ and $$(III)$$

$$(I)$$ and $$(IV)$$

$$(II), (III)$$ and $$(IV)$$

Solution

Question 4

Increases

Decreases

Remains constant

Nothing can be said

Solution

Question 5

$$292.0\ K$$

$$298.0\ K$$

$$290.8\ K$$

$$293.7\ K$$

Solution

Question 6

$$0^{0}C$$

$$4^{0}C$$

$$- 4^{0}C$$

$$- 2^{0}C$$

Solution

Question 7

1

0

4

6

Solution

Question 8

one-third

equal

half

double

Solution

Question 9

heat capacity at constant volume

heat capacity at constant pressure

heat capacity mol$$^{-1}$$

heat capacity g$$^{-1}$$

Solution

Question 10

462.12 K

362.12 k

262.12 k

562.12 k

Solution

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$$C(diamond)), C(graphite), Br_2(I)
$$

$$C(graphite), Br_2(I), I_2(s)
$$