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Thermodynamics

148488 during adiabatic expansion of 2 moles of a gas, the change in internal energy was found to be equal to $100 J$ . The work done during the process will be equal to

1 Zero

2

200 J

3

- 100 J

4

100 J

Explanation:

D according to first law
$Δ Q = W + Δ U$
during adiabatic expansion ${Δ Q = 0}$
$W + Δ U = 0$
$W = - Δ U$
$W = - (- 100)$
$W = 100 J$

AP EAMCET-25.09.2020

Thermodynamics

148489 When the ideal gas is compressed isothermally, then its pressure

1 Increases

2 Decreases

3 remains the same

4 first increases and then decreases

Explanation:

A When the ideal gas is compressed isothermally $(T = C)$
Then the volume of gas gets decreases
As we know,
$PV = nRT$
$T = C$
$PV = Constant$
$P \propto \frac{1}{V}$
Volume decreases, when compressed isothermally then pressure will increase.
Hence, it is said that when ideal gas is compressed isothermally the pressure will increase.

AP EAMCET-24.08.2021

Thermodynamics

148490 A given system undergoes a change in which the work done by the system equals the decrease in its internal energy. The system must have undergone an

1 Isothermal change

2 Adiabatic change

3 Isobaric change

4 Isochoric change

Explanation:

B We know that,
$Δ W + Δ U = 0$
$Δ W = - Δ U$
According to first law of thermodynamics
$Δ Q = Δ U + Δ W$
$Δ Q = 0$
( $∵$ adiabatic process)
$Δ U = - Δ W$
$Δ W = - Δ U$
Hence, process is adiabatic.

AP EAMCET-25.08.2021

Thermodynamics

148491 The mole of an ideal gas expands adiabatically from $200 K$ to $250 K$ . If the specific heat of the gas at constant volume is $0.8 kJ {kg}^{- 1}$ , then the work done by the gas is

1

20 J

2

20 kJ

3

40 J

4

40 kJ

Explanation:

D Given,
Temperature change $= 250 K - 200 K = 50 K$
Specific heat $= 0.8 kJ / kg$
$dU = ms Δ T$
$dU = 1 \times 0.8 \times 50$
$dU = 40 kJ$
As we know that,
$dQ = dU + dW$
$dW = - dU$
$dW = - 40 [dQ = 0 for adiabatic process]$
Work done by the gas $= 40 kJ$ .

AP EAMCET-24.04.2017

Thermodynamics

148488 during adiabatic expansion of 2 moles of a gas, the change in internal energy was found to be equal to $100 J$ . The work done during the process will be equal to

1 Zero

2

200 J

3

- 100 J

4

100 J

Explanation:

D according to first law
$Δ Q = W + Δ U$
during adiabatic expansion ${Δ Q = 0}$
$W + Δ U = 0$
$W = - Δ U$
$W = - (- 100)$
$W = 100 J$

AP EAMCET-25.09.2020

Thermodynamics

148489 When the ideal gas is compressed isothermally, then its pressure

1 Increases

2 Decreases

3 remains the same

4 first increases and then decreases

Explanation:

A When the ideal gas is compressed isothermally $(T = C)$
Then the volume of gas gets decreases
As we know,
$PV = nRT$
$T = C$
$PV = Constant$
$P \propto \frac{1}{V}$
Volume decreases, when compressed isothermally then pressure will increase.
Hence, it is said that when ideal gas is compressed isothermally the pressure will increase.

AP EAMCET-24.08.2021

Thermodynamics

148490 A given system undergoes a change in which the work done by the system equals the decrease in its internal energy. The system must have undergone an

1 Isothermal change

2 Adiabatic change

3 Isobaric change

4 Isochoric change

Explanation:

B We know that,
$Δ W + Δ U = 0$
$Δ W = - Δ U$
According to first law of thermodynamics
$Δ Q = Δ U + Δ W$
$Δ Q = 0$
( $∵$ adiabatic process)
$Δ U = - Δ W$
$Δ W = - Δ U$
Hence, process is adiabatic.

AP EAMCET-25.08.2021

Thermodynamics

148491 The mole of an ideal gas expands adiabatically from $200 K$ to $250 K$ . If the specific heat of the gas at constant volume is $0.8 kJ {kg}^{- 1}$ , then the work done by the gas is

1

20 J

2

20 kJ

3

40 J

4

40 kJ

Explanation:

D Given,
Temperature change $= 250 K - 200 K = 50 K$
Specific heat $= 0.8 kJ / kg$
$dU = ms Δ T$
$dU = 1 \times 0.8 \times 50$
$dU = 40 kJ$
As we know that,
$dQ = dU + dW$
$dW = - dU$
$dW = - 40 [dQ = 0 for adiabatic process]$
Work done by the gas $= 40 kJ$ .

AP EAMCET-24.04.2017

Thermodynamics

148488 during adiabatic expansion of 2 moles of a gas, the change in internal energy was found to be equal to $100 J$ . The work done during the process will be equal to

1 Zero

2

200 J

3

- 100 J

4

100 J

Explanation:

D according to first law
$Δ Q = W + Δ U$
during adiabatic expansion ${Δ Q = 0}$
$W + Δ U = 0$
$W = - Δ U$
$W = - (- 100)$
$W = 100 J$

AP EAMCET-25.09.2020

Thermodynamics

148489 When the ideal gas is compressed isothermally, then its pressure

1 Increases

2 Decreases

3 remains the same

4 first increases and then decreases

Explanation:

A When the ideal gas is compressed isothermally $(T = C)$
Then the volume of gas gets decreases
As we know,
$PV = nRT$
$T = C$
$PV = Constant$
$P \propto \frac{1}{V}$
Volume decreases, when compressed isothermally then pressure will increase.
Hence, it is said that when ideal gas is compressed isothermally the pressure will increase.

AP EAMCET-24.08.2021

Thermodynamics

148490 A given system undergoes a change in which the work done by the system equals the decrease in its internal energy. The system must have undergone an

1 Isothermal change

2 Adiabatic change

3 Isobaric change

4 Isochoric change

Explanation:

B We know that,
$Δ W + Δ U = 0$
$Δ W = - Δ U$
According to first law of thermodynamics
$Δ Q = Δ U + Δ W$
$Δ Q = 0$
( $∵$ adiabatic process)
$Δ U = - Δ W$
$Δ W = - Δ U$
Hence, process is adiabatic.

AP EAMCET-25.08.2021

Thermodynamics

148491 The mole of an ideal gas expands adiabatically from $200 K$ to $250 K$ . If the specific heat of the gas at constant volume is $0.8 kJ {kg}^{- 1}$ , then the work done by the gas is

1

20 J

2

20 kJ

3

40 J

4

40 kJ

Explanation:

D Given,
Temperature change $= 250 K - 200 K = 50 K$
Specific heat $= 0.8 kJ / kg$
$dU = ms Δ T$
$dU = 1 \times 0.8 \times 50$
$dU = 40 kJ$
As we know that,
$dQ = dU + dW$
$dW = - dU$
$dW = - 40 [dQ = 0 for adiabatic process]$
Work done by the gas $= 40 kJ$ .

AP EAMCET-24.04.2017

Thermodynamics

148488 during adiabatic expansion of 2 moles of a gas, the change in internal energy was found to be equal to $100 J$ . The work done during the process will be equal to

1 Zero

2

200 J

3

- 100 J

4

100 J

Explanation:

D according to first law
$Δ Q = W + Δ U$
during adiabatic expansion ${Δ Q = 0}$
$W + Δ U = 0$
$W = - Δ U$
$W = - (- 100)$
$W = 100 J$

AP EAMCET-25.09.2020

Thermodynamics

148489 When the ideal gas is compressed isothermally, then its pressure

1 Increases

2 Decreases

3 remains the same

4 first increases and then decreases

Explanation:

A When the ideal gas is compressed isothermally $(T = C)$
Then the volume of gas gets decreases
As we know,
$PV = nRT$
$T = C$
$PV = Constant$
$P \propto \frac{1}{V}$
Volume decreases, when compressed isothermally then pressure will increase.
Hence, it is said that when ideal gas is compressed isothermally the pressure will increase.

AP EAMCET-24.08.2021

Thermodynamics

148490 A given system undergoes a change in which the work done by the system equals the decrease in its internal energy. The system must have undergone an

1 Isothermal change

2 Adiabatic change

3 Isobaric change

4 Isochoric change

Explanation:

B We know that,
$Δ W + Δ U = 0$
$Δ W = - Δ U$
According to first law of thermodynamics
$Δ Q = Δ U + Δ W$
$Δ Q = 0$
( $∵$ adiabatic process)
$Δ U = - Δ W$
$Δ W = - Δ U$
Hence, process is adiabatic.

AP EAMCET-25.08.2021

Thermodynamics

148491 The mole of an ideal gas expands adiabatically from $200 K$ to $250 K$ . If the specific heat of the gas at constant volume is $0.8 kJ {kg}^{- 1}$ , then the work done by the gas is

1

20 J

2

20 kJ

3

40 J

4

40 kJ

Explanation:

D Given,
Temperature change $= 250 K - 200 K = 50 K$
Specific heat $= 0.8 kJ / kg$
$dU = ms Δ T$
$dU = 1 \times 0.8 \times 50$
$dU = 40 kJ$
As we know that,
$dQ = dU + dW$
$dW = - dU$
$dW = - 40 [dQ = 0 for adiabatic process]$
Work done by the gas $= 40 kJ$ .

AP EAMCET-24.04.2017