Thermodynamics Test

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Thermodynamics Test - 74

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Weekly Quiz Competition

Question 1
1 / -0

One mole of a monoatomic gas is heated at a constant pressure of $1atm$ from $0K$ to $100K$ . If the gas constant $R=8.32J{mol}^{-1}{K}^{-1}$ , the change in the internal energy of the gas is approximately

A
$2.3J$

B
$46J$

C
$8.67\times{10}^{3}J$

D
$1.25\times{10}^{3}J$

Solution
Question 2
1 / -0

Ethyl chloride $(C_{2}H_{5}Cl)$ is prepared by:-

$C_{2}H_{4(g)}+HCl_{(g)}\rightarrow C_{2}H_{5}Cl_{(g)};\ \ \Delta H=-72.3 kJ$ if 98 g of $C_{2}H_{4}$ and 109.5 g $HCl$ are used at 300 K, then find $\Delta E$ .

A
-64.8 kJ

B
-190 kJ

C
209.4 kJ

D
-209.4 kJ

Solution
Question 3
1 / -0

A gas is compressed at a constant pressure of 50 $N/m^{ 2 }$ from a volume of $10m^{ 3 }$ to a volume of $4m^{ 3 }$ . Energy of 100 J is then added to the gas by heating. Its internal energy is

A
increased by 400 J

B
increased by 200 J

C
increased by 100 J

D
decreased by 400 J

Solution
Question 4
1 / -0

The enthaply change on freezing of $1\ mol$ of water at $10^ {o}C$ to ice at $-10^ {o}C$ is:

A
$6.56\ kJ\ mol^ {-1}$

B
$5.81\ kJ\ mol^ {-1}$

C
$6.00\ kJ\ mol^ {-1}$

D
$5.64\ kJ\ mol^ {-1}$
Question 5
1 / -0

Which relationship is incorrect? (for reversible isothermal process)

A
$\Delta H=\Delta U+\Delta n_{g}$ RT(for reaction)

B
$\Delta G= T \Delta S$

C
$\Delta G^{\circ}=-2.303$ RT log K

D
W= +2.303 nRT log $\frac{V_{1}}{V_{2}}$

Solution
Question 6
1 / -0

The internal energy of an ideal gas increases when it

A
Expands

B
Is compressed

C
Is first expanded and then compressed

D
None of these

Solution
Question 7
1 / -0

The amount of heat required to raise the temperature of 1 mole diatomic gas by $1^0C$ a constant pressure is 60 cal. The amount of heat which goes as internal energy of the gas is nearly

A
60 cal

B
30 cal

C
42.6 cal

D
49.8 cal

Solution
Question 8
1 / -0

A reaction is spontaneous at low temperature but non-spontaneous at high temperature. Which of the following is true for the reaction?

A
$\triangle H > 0,\triangle S > 0$

B
$\triangle H < 0,\triangle S > 0$

C
$\triangle H > 0,\triangle S=0$

D
$\triangle H < 0,\triangle S < 0$

E
$\triangle H = 0,\triangle S < 0$

Solution
Question 9
1 / -0

Energy required to dissociate, 16 g oxygen gas into free atom is x kJ. The heat of atomisation of oxygen is :-

A
x/2

B
2x

C
x

D
16
Question 10
1 / -0

In a thermodynamic process, pressure of a fixed mass of a gas is changed in such a manner that the gas molecules gives out 20 J of heat and 10 J of work is done on the gas. If the initial internal energy of the gas was 40 J, then the final internal energy will be

A
$30 J$

B
$20 J$

C
$60 J$

D
$40 J$

Solution

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Re-Attempt Weekly Quiz Competition

Thermodynamics Test - 74

Result

Thermodynamics Test - 74

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SHARING IS CARING

Question 1

2.3J2.3J2.3J

46J46J46J

8.67×103J8.67\times{10}^{3}J8.67×103J

1.25×103J1.25\times{10}^{3}J1.25×103J

Solution

Question 2

-64.8 kJ

-190 kJ

209.4 kJ

-209.4 kJ

Solution

Question 3

increased by 400 J

increased by 200 J

increased by 100 J

decreased by 400 J

Solution

Question 4

6.56 kJ mol−16.56\ kJ\ mol^ {-1}6.56 kJ mol−1

5.81 kJ mol−15.81\ kJ\ mol^ {-1}5.81 kJ mol−1

6.00 kJ mol−16.00\ kJ\ mol^ {-1}6.00 kJ mol−1

5.64 kJ mol−15.64\ kJ\ mol^ {-1}5.64 kJ mol−1

Question 5

ΔH=ΔU+Δng\Delta H=\Delta U+\Delta n_{g}ΔH=ΔU+Δng​ RT(for reaction)

ΔG=TΔS\Delta G= T \Delta SΔG=TΔS

ΔG∘=−2.303\Delta G^{\circ}=-2.303ΔG∘=−2.303 RT log K

W= +2.303 nRT log V1V2\frac{V_{1}}{V_{2}}V2​V1​​

Solution

Question 6

Expands

Is compressed

Is first expanded and then compressed

None of these

Solution

Question 7

60 cal

30 cal

42.6 cal

49.8 cal

Solution

Question 8

△H>0,△S>0\triangle H > 0,\triangle S > 0△H>0,△S>0

△H<0,△S>0\triangle H < 0,\triangle S > 0△H<0,△S>0

△H>0,△S=0\triangle H > 0,\triangle S=0△H>0,△S=0

△H<0,△S<0\triangle H < 0,\triangle S < 0△H<0,△S<0

△H=0,△S<0\triangle H = 0,\triangle S < 0△H=0,△S<0

Solution

Question 9

x/2

2x

x

16

Question 10

30J30 J30J

20J20 J20J

60J60 J60J

40J40 J40J

Solution

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$2.3J$

$46J$

$8.67\times{10}^{3}J$

$1.25\times{10}^{3}J$

$6.56\ kJ\ mol^ {-1}$

$5.81\ kJ\ mol^ {-1}$

$6.00\ kJ\ mol^ {-1}$

$5.64\ kJ\ mol^ {-1}$

$\Delta H=\Delta U+\Delta n_{g}$ RT(for reaction)

$\Delta G= T \Delta S$

$\Delta G^{\circ}=-2.303$ RT log K

W= +2.303 nRT log $\frac{V_{1}}{V_{2}}$

$\triangle H > 0,\triangle S > 0$

$\triangle H < 0,\triangle S > 0$

$\triangle H > 0,\triangle S=0$

$\triangle H < 0,\triangle S < 0$

$\triangle H = 0,\triangle S < 0$

$30 J$

$20 J$

$60 J$

$40 J$