QBManager

Thermodynamics

148452 In an adiabatic expansion of an ideal gas the product of pressure and volume :

1 decreases

2 increases

3 remains constant

4 at first increases and then decreases

Explanation:

A Ideal gas equation is given by,
$PV = nRT$
$∵ T$ is decreasing, $PV$ also decreases.
If $T$ decreases $PV$ also decreases because in an adiabatic expansion. Internal energy decreases and temperature also decreases.

Karnataka CET-2020

Thermodynamics

148461 In an adiabatic process

1

P^{γ} V =

constant

2

{TV}^{γ - 1} =

constant

3

PV =

constant

4 All of these

Explanation:

B For an adiabatic process, ${PV}^{γ} =$ constant.
Using the ideal gas equation and substituting $V = \frac{nRT}{P}$ In the above equation gives ${TV}^{γ - 1} =$ constant
Where $γ$ is the specific heat ratio

UP CPMT-2003

Thermodynamics

148463 During adiabatic expansion, the increase in the volume is associated with

1 increase in pressure and decrease in

T

2 decrease in pressure and increase in

T

3 increase in pressure and

T

4 decrease in pressure and

T

Explanation:

D ${PV}^{γ} =$ constant
And, ${TV}^{γ - 1} =$ constant
From the above equation increasing in volume pressure and temperature both are decreases.

TS EAMCET 30.07.2022

Thermodynamics

148464 An ideal gas undergoes an adiabatic process. If the pressure of the gas is reduced by $0.1 %$ then the volume is changed by $($ Given $γ = \frac{C_{p}}{C_{v}} = 5 / 3)$

1

0.1 %

2

0.05 %

3

0.06 %

4

- 0.05 %

Explanation:

C From the relation, ${PV}^{γ} = K$
Now differentiating we get, ${PV}^{γ - 1} dV + dP \cdot V^{γ} = 0$
By making proper rearrangements we get, $\frac{- dV}{V} = \frac{dP}{γ P}$ In adiabatic process on a gas with $γ = 1.4$ , the pressure of the is reduced by $0.1 %$ .
The volume (decreases) changes by about,
$\frac{- dV}{V} = \frac{0.1}{1.4} \times 100 = 0.06 %$

TS EAMCET 05.08.2021

Thermodynamics

148496 A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then

1 compressing the gas through adiabatic process will require more work to be done.

2 compressing the gas isothermally or adiabatically will require the same amount of work.

3 which of the case (whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.

4 compressing the gas isothermally will require more work to be done.

Explanation:

A
Let us consider that the gas undergoes compression from $V$ to $\frac{V}{2}$ .
From $P - V$ diagram, when we compare the area under the isothermal process curve and the adiabatic process curve, the work done for adiabatic process is higher than that of work done by isothermal process.

NEET-2016

Thermodynamics

148452 In an adiabatic expansion of an ideal gas the product of pressure and volume :

1 decreases

2 increases

3 remains constant

4 at first increases and then decreases

Explanation:

A Ideal gas equation is given by,
$PV = nRT$
$∵ T$ is decreasing, $PV$ also decreases.
If $T$ decreases $PV$ also decreases because in an adiabatic expansion. Internal energy decreases and temperature also decreases.

Karnataka CET-2020

Thermodynamics

148461 In an adiabatic process

1

P^{γ} V =

constant

2

{TV}^{γ - 1} =

constant

3

PV =

constant

4 All of these

Explanation:

B For an adiabatic process, ${PV}^{γ} =$ constant.
Using the ideal gas equation and substituting $V = \frac{nRT}{P}$ In the above equation gives ${TV}^{γ - 1} =$ constant
Where $γ$ is the specific heat ratio

UP CPMT-2003

Thermodynamics

148463 During adiabatic expansion, the increase in the volume is associated with

1 increase in pressure and decrease in

T

2 decrease in pressure and increase in

T

3 increase in pressure and

T

4 decrease in pressure and

T

Explanation:

D ${PV}^{γ} =$ constant
And, ${TV}^{γ - 1} =$ constant
From the above equation increasing in volume pressure and temperature both are decreases.

TS EAMCET 30.07.2022

Thermodynamics

148464 An ideal gas undergoes an adiabatic process. If the pressure of the gas is reduced by $0.1 %$ then the volume is changed by $($ Given $γ = \frac{C_{p}}{C_{v}} = 5 / 3)$

1

0.1 %

2

0.05 %

3

0.06 %

4

- 0.05 %

Explanation:

C From the relation, ${PV}^{γ} = K$
Now differentiating we get, ${PV}^{γ - 1} dV + dP \cdot V^{γ} = 0$
By making proper rearrangements we get, $\frac{- dV}{V} = \frac{dP}{γ P}$ In adiabatic process on a gas with $γ = 1.4$ , the pressure of the is reduced by $0.1 %$ .
The volume (decreases) changes by about,
$\frac{- dV}{V} = \frac{0.1}{1.4} \times 100 = 0.06 %$

TS EAMCET 05.08.2021

Thermodynamics

148496 A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then

1 compressing the gas through adiabatic process will require more work to be done.

2 compressing the gas isothermally or adiabatically will require the same amount of work.

3 which of the case (whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.

4 compressing the gas isothermally will require more work to be done.

Explanation:

A
Let us consider that the gas undergoes compression from $V$ to $\frac{V}{2}$ .
From $P - V$ diagram, when we compare the area under the isothermal process curve and the adiabatic process curve, the work done for adiabatic process is higher than that of work done by isothermal process.

NEET-2016

Thermodynamics

148452 In an adiabatic expansion of an ideal gas the product of pressure and volume :

1 decreases

2 increases

3 remains constant

4 at first increases and then decreases

Explanation:

A Ideal gas equation is given by,
$PV = nRT$
$∵ T$ is decreasing, $PV$ also decreases.
If $T$ decreases $PV$ also decreases because in an adiabatic expansion. Internal energy decreases and temperature also decreases.

Karnataka CET-2020

Thermodynamics

148461 In an adiabatic process

1

P^{γ} V =

constant

2

{TV}^{γ - 1} =

constant

3

PV =

constant

4 All of these

Explanation:

B For an adiabatic process, ${PV}^{γ} =$ constant.
Using the ideal gas equation and substituting $V = \frac{nRT}{P}$ In the above equation gives ${TV}^{γ - 1} =$ constant
Where $γ$ is the specific heat ratio

UP CPMT-2003

Thermodynamics

148463 During adiabatic expansion, the increase in the volume is associated with

1 increase in pressure and decrease in

T

2 decrease in pressure and increase in

T

3 increase in pressure and

T

4 decrease in pressure and

T

Explanation:

D ${PV}^{γ} =$ constant
And, ${TV}^{γ - 1} =$ constant
From the above equation increasing in volume pressure and temperature both are decreases.

TS EAMCET 30.07.2022

Thermodynamics

148464 An ideal gas undergoes an adiabatic process. If the pressure of the gas is reduced by $0.1 %$ then the volume is changed by $($ Given $γ = \frac{C_{p}}{C_{v}} = 5 / 3)$

1

0.1 %

2

0.05 %

3

0.06 %

4

- 0.05 %

Explanation:

C From the relation, ${PV}^{γ} = K$
Now differentiating we get, ${PV}^{γ - 1} dV + dP \cdot V^{γ} = 0$
By making proper rearrangements we get, $\frac{- dV}{V} = \frac{dP}{γ P}$ In adiabatic process on a gas with $γ = 1.4$ , the pressure of the is reduced by $0.1 %$ .
The volume (decreases) changes by about,
$\frac{- dV}{V} = \frac{0.1}{1.4} \times 100 = 0.06 %$

TS EAMCET 05.08.2021

Thermodynamics

148496 A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then

1 compressing the gas through adiabatic process will require more work to be done.

2 compressing the gas isothermally or adiabatically will require the same amount of work.

3 which of the case (whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.

4 compressing the gas isothermally will require more work to be done.

Explanation:

A
Let us consider that the gas undergoes compression from $V$ to $\frac{V}{2}$ .
From $P - V$ diagram, when we compare the area under the isothermal process curve and the adiabatic process curve, the work done for adiabatic process is higher than that of work done by isothermal process.

NEET-2016

Thermodynamics

148452 In an adiabatic expansion of an ideal gas the product of pressure and volume :

1 decreases

2 increases

3 remains constant

4 at first increases and then decreases

Explanation:

A Ideal gas equation is given by,
$PV = nRT$
$∵ T$ is decreasing, $PV$ also decreases.
If $T$ decreases $PV$ also decreases because in an adiabatic expansion. Internal energy decreases and temperature also decreases.

Karnataka CET-2020

Thermodynamics

148461 In an adiabatic process

1

P^{γ} V =

constant

2

{TV}^{γ - 1} =

constant

3

PV =

constant

4 All of these

Explanation:

B For an adiabatic process, ${PV}^{γ} =$ constant.
Using the ideal gas equation and substituting $V = \frac{nRT}{P}$ In the above equation gives ${TV}^{γ - 1} =$ constant
Where $γ$ is the specific heat ratio

UP CPMT-2003

Thermodynamics

148463 During adiabatic expansion, the increase in the volume is associated with

1 increase in pressure and decrease in

T

2 decrease in pressure and increase in

T

3 increase in pressure and

T

4 decrease in pressure and

T

Explanation:

D ${PV}^{γ} =$ constant
And, ${TV}^{γ - 1} =$ constant
From the above equation increasing in volume pressure and temperature both are decreases.

TS EAMCET 30.07.2022

Thermodynamics

148464 An ideal gas undergoes an adiabatic process. If the pressure of the gas is reduced by $0.1 %$ then the volume is changed by $($ Given $γ = \frac{C_{p}}{C_{v}} = 5 / 3)$

1

0.1 %

2

0.05 %

3

0.06 %

4

- 0.05 %

Explanation:

C From the relation, ${PV}^{γ} = K$
Now differentiating we get, ${PV}^{γ - 1} dV + dP \cdot V^{γ} = 0$
By making proper rearrangements we get, $\frac{- dV}{V} = \frac{dP}{γ P}$ In adiabatic process on a gas with $γ = 1.4$ , the pressure of the is reduced by $0.1 %$ .
The volume (decreases) changes by about,
$\frac{- dV}{V} = \frac{0.1}{1.4} \times 100 = 0.06 %$

TS EAMCET 05.08.2021

Thermodynamics

148496 A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then

1 compressing the gas through adiabatic process will require more work to be done.

2 compressing the gas isothermally or adiabatically will require the same amount of work.

3 which of the case (whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.

4 compressing the gas isothermally will require more work to be done.

Explanation:

A
Let us consider that the gas undergoes compression from $V$ to $\frac{V}{2}$ .
From $P - V$ diagram, when we compare the area under the isothermal process curve and the adiabatic process curve, the work done for adiabatic process is higher than that of work done by isothermal process.

NEET-2016

Thermodynamics

148452 In an adiabatic expansion of an ideal gas the product of pressure and volume :

1 decreases

2 increases

3 remains constant

4 at first increases and then decreases

Explanation:

A Ideal gas equation is given by,
$PV = nRT$
$∵ T$ is decreasing, $PV$ also decreases.
If $T$ decreases $PV$ also decreases because in an adiabatic expansion. Internal energy decreases and temperature also decreases.

Karnataka CET-2020

Thermodynamics

148461 In an adiabatic process

1

P^{γ} V =

constant

2

{TV}^{γ - 1} =

constant

3

PV =

constant

4 All of these

Explanation:

B For an adiabatic process, ${PV}^{γ} =$ constant.
Using the ideal gas equation and substituting $V = \frac{nRT}{P}$ In the above equation gives ${TV}^{γ - 1} =$ constant
Where $γ$ is the specific heat ratio

UP CPMT-2003

Thermodynamics

148463 During adiabatic expansion, the increase in the volume is associated with

1 increase in pressure and decrease in

T

2 decrease in pressure and increase in

T

3 increase in pressure and

T

4 decrease in pressure and

T

Explanation:

D ${PV}^{γ} =$ constant
And, ${TV}^{γ - 1} =$ constant
From the above equation increasing in volume pressure and temperature both are decreases.

TS EAMCET 30.07.2022

Thermodynamics

148464 An ideal gas undergoes an adiabatic process. If the pressure of the gas is reduced by $0.1 %$ then the volume is changed by $($ Given $γ = \frac{C_{p}}{C_{v}} = 5 / 3)$

1

0.1 %

2

0.05 %

3

0.06 %

4

- 0.05 %

Explanation:

C From the relation, ${PV}^{γ} = K$
Now differentiating we get, ${PV}^{γ - 1} dV + dP \cdot V^{γ} = 0$
By making proper rearrangements we get, $\frac{- dV}{V} = \frac{dP}{γ P}$ In adiabatic process on a gas with $γ = 1.4$ , the pressure of the is reduced by $0.1 %$ .
The volume (decreases) changes by about,
$\frac{- dV}{V} = \frac{0.1}{1.4} \times 100 = 0.06 %$

TS EAMCET 05.08.2021

Thermodynamics

148496 A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then

1 compressing the gas through adiabatic process will require more work to be done.

2 compressing the gas isothermally or adiabatically will require the same amount of work.

3 which of the case (whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas.

4 compressing the gas isothermally will require more work to be done.

Explanation:

A
Let us consider that the gas undergoes compression from $V$ to $\frac{V}{2}$ .
From $P - V$ diagram, when we compare the area under the isothermal process curve and the adiabatic process curve, the work done for adiabatic process is higher than that of work done by isothermal process.

NEET-2016

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Question Bank Series

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation: