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CHXI06:THERMODYNAMICS

369313 A system does $394 J$ of work on surrounding by absorbing $701 J$ heat. What is the change in internal energy of the system?

1

547 J

2

1095 J

3

307 J

4

394 J

Explanation:

$W = - 394 J ($ work done by the system),
$Q = 701 J$ (heat absorbed)
According to first law of thermodynamics
$Δ U = Q + W$
$= 701 - 394 = 307 J$

MHTCET - 2021

CHXI06:THERMODYNAMICS

369314 Assertion :
First law of thermodynamics is applicable to an electric fan or a heater.
Reason :
In an electric fan, the electrical energy is converted into chemical work that moves the blades. In a heater, electrical energy is converted into heat energy.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

CHXI06:THERMODYNAMICS

369315 Assertion :
For an isothermal reversible process, $q = - w$ i.e.,work done by the system equals the heat absorbed by the system.
Reason :
Enthalpy change $(Δ H)$ is not zero for isothermal process.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In an isothermal process, there is no change in the internal energy $(U)$ as it is a function of temperature. Therefore, $Δ U$ is zero.
According to the first law of thermodynamics, $q + w = Δ U$ , this implies that if $Δ U$ is $0, q + w$ $= 0$ . Therefore, when $(Δ U = 0), - w = q$ . Thus work done by the system is equal to the heat absorbed by the system. Thus, option (3) is correct.

CHXI06:THERMODYNAMICS

369316 A system absorbs $10 kJ$ of heat and does $4 kJ$ of work. The internal energy of the system

1 Decreases by

6 kJ

2 Increases by

6 kJ

3 Decreases by

14 kJ

4 Increases by

14 kJ

Explanation:

$q = + 10 k J, w = - 4 k J$
$Δ U = q + w = 10 - 4 = 6 kJ$

CHXI06:THERMODYNAMICS

369313 A system does $394 J$ of work on surrounding by absorbing $701 J$ heat. What is the change in internal energy of the system?

1

547 J

2

1095 J

3

307 J

4

394 J

Explanation:

$W = - 394 J ($ work done by the system),
$Q = 701 J$ (heat absorbed)
According to first law of thermodynamics
$Δ U = Q + W$
$= 701 - 394 = 307 J$

MHTCET - 2021

CHXI06:THERMODYNAMICS

369314 Assertion :
First law of thermodynamics is applicable to an electric fan or a heater.
Reason :
In an electric fan, the electrical energy is converted into chemical work that moves the blades. In a heater, electrical energy is converted into heat energy.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

CHXI06:THERMODYNAMICS

369315 Assertion :
For an isothermal reversible process, $q = - w$ i.e.,work done by the system equals the heat absorbed by the system.
Reason :
Enthalpy change $(Δ H)$ is not zero for isothermal process.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In an isothermal process, there is no change in the internal energy $(U)$ as it is a function of temperature. Therefore, $Δ U$ is zero.
According to the first law of thermodynamics, $q + w = Δ U$ , this implies that if $Δ U$ is $0, q + w$ $= 0$ . Therefore, when $(Δ U = 0), - w = q$ . Thus work done by the system is equal to the heat absorbed by the system. Thus, option (3) is correct.

CHXI06:THERMODYNAMICS

369316 A system absorbs $10 kJ$ of heat and does $4 kJ$ of work. The internal energy of the system

1 Decreases by

6 kJ

2 Increases by

6 kJ

3 Decreases by

14 kJ

4 Increases by

14 kJ

Explanation:

$q = + 10 k J, w = - 4 k J$
$Δ U = q + w = 10 - 4 = 6 kJ$

CHXI06:THERMODYNAMICS

369313 A system does $394 J$ of work on surrounding by absorbing $701 J$ heat. What is the change in internal energy of the system?

1

547 J

2

1095 J

3

307 J

4

394 J

Explanation:

$W = - 394 J ($ work done by the system),
$Q = 701 J$ (heat absorbed)
According to first law of thermodynamics
$Δ U = Q + W$
$= 701 - 394 = 307 J$

MHTCET - 2021

CHXI06:THERMODYNAMICS

369314 Assertion :
First law of thermodynamics is applicable to an electric fan or a heater.
Reason :
In an electric fan, the electrical energy is converted into chemical work that moves the blades. In a heater, electrical energy is converted into heat energy.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

CHXI06:THERMODYNAMICS

369315 Assertion :
For an isothermal reversible process, $q = - w$ i.e.,work done by the system equals the heat absorbed by the system.
Reason :
Enthalpy change $(Δ H)$ is not zero for isothermal process.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In an isothermal process, there is no change in the internal energy $(U)$ as it is a function of temperature. Therefore, $Δ U$ is zero.
According to the first law of thermodynamics, $q + w = Δ U$ , this implies that if $Δ U$ is $0, q + w$ $= 0$ . Therefore, when $(Δ U = 0), - w = q$ . Thus work done by the system is equal to the heat absorbed by the system. Thus, option (3) is correct.

CHXI06:THERMODYNAMICS

369316 A system absorbs $10 kJ$ of heat and does $4 kJ$ of work. The internal energy of the system

1 Decreases by

6 kJ

2 Increases by

6 kJ

3 Decreases by

14 kJ

4 Increases by

14 kJ

Explanation:

$q = + 10 k J, w = - 4 k J$
$Δ U = q + w = 10 - 4 = 6 kJ$

CHXI06:THERMODYNAMICS

369313 A system does $394 J$ of work on surrounding by absorbing $701 J$ heat. What is the change in internal energy of the system?

1

547 J

2

1095 J

3

307 J

4

394 J

Explanation:

$W = - 394 J ($ work done by the system),
$Q = 701 J$ (heat absorbed)
According to first law of thermodynamics
$Δ U = Q + W$
$= 701 - 394 = 307 J$

MHTCET - 2021

CHXI06:THERMODYNAMICS

369314 Assertion :
First law of thermodynamics is applicable to an electric fan or a heater.
Reason :
In an electric fan, the electrical energy is converted into chemical work that moves the blades. In a heater, electrical energy is converted into heat energy.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

CHXI06:THERMODYNAMICS

369315 Assertion :
For an isothermal reversible process, $q = - w$ i.e.,work done by the system equals the heat absorbed by the system.
Reason :
Enthalpy change $(Δ H)$ is not zero for isothermal process.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

Explanation:

In an isothermal process, there is no change in the internal energy $(U)$ as it is a function of temperature. Therefore, $Δ U$ is zero.
According to the first law of thermodynamics, $q + w = Δ U$ , this implies that if $Δ U$ is $0, q + w$ $= 0$ . Therefore, when $(Δ U = 0), - w = q$ . Thus work done by the system is equal to the heat absorbed by the system. Thus, option (3) is correct.

CHXI06:THERMODYNAMICS

369316 A system absorbs $10 kJ$ of heat and does $4 kJ$ of work. The internal energy of the system

1 Decreases by

6 kJ

2 Increases by

6 kJ

3 Decreases by

14 kJ

4 Increases by

14 kJ

Explanation:

$q = + 10 k J, w = - 4 k J$
$Δ U = q + w = 10 - 4 = 6 kJ$

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