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PHXI12:THERMODYNAMICS

371478 In which of the following processes, heat is neither absorbed nor released by a system?

1 Isothermal

2 Adiabatic

3 Isobaric

4 Isochoric

NEET - 2019

PHXI12:THERMODYNAMICS

371479 Assertion :
An adiabatic process is an isoentropic process.
Reason :
Change in entropy is zero in case of adiabatic process.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

In adiabatic process $Δ S = \frac{Δ Q}{T} = 0$ , since there is no heat exchange $(Δ Q = 0)$ (with the surroundings).
$\Rightarrow S =$ constant
So, this process is called isentropic
So correct option is (1).

PHXI12:THERMODYNAMICS

371480 Assertion :
Work done by a gas in isothermal expansion is more than the work done by the gas in the same expansion, adiabatically.
Reason :
Temperature remains constant in isothermal expansion and not in adiabatic expansion.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

Adiabatic $Δ Q = 0$
$\Rightarrow | Δ U | = | Δ W |$ (by first law of thermodynamics) Isothermal $Δ T = 0$
$\Rightarrow Δ Q = Δ W$
$\Rightarrow$ complete $Δ Q$ is used as work in isothermal.
$\Rightarrow$ work done in isothermal expansion is greater than in adiabatic expansion. However, the reason lacks precision, attributing the difference to temperature alone, while it's influenced by the change in internal energy. So correct option is (2).

PHXI12:THERMODYNAMICS

371481 $Δ U + Δ W = 0$ is valid for

1 Isothermal process

2 Adiabatic process

3 Isochoric process

4 Isobaric process

Explanation:

In adiabatic process
$\begin{aligned} Δ Q = 0 \Rightarrow Δ U + Δ W = 0 \\ (∵ Δ Q = Δ U + Δ W) \end{aligned}$

PHXI12:THERMODYNAMICS

371482 A tyre pumped to a pressure $3.375 atm$ at $27^{\circ} C$ suddenly bursts. What is the final temperature $(γ = 1.5)$ ?

1

- 27^{\circ} C

2

27^{\circ} C

3

- 73^{\circ} C

4

0^{\circ} C

Explanation:

Sudden bursting of a tyre can be treated as adiabatic expansion
$T_{1}^{γ} P_{1}^{1 - γ} = T_{2}^{γ} P_{2}^{1 - γ}$
${(\frac{T_{1}}{T_{2}})}^{γ} = {(\frac{P_{1}}{P_{2}})}^{γ - 1} \Rightarrow {(\frac{300}{T_{2}})}^{3 / 2} = {(\frac{3.375}{1})}^{3 / 2 - 1}$
$T_{2} = \frac{300}{{(3.375)}^{1 / 3}} = 200 K = - 73^{\circ} C$

PHXI12:THERMODYNAMICS

371478 In which of the following processes, heat is neither absorbed nor released by a system?

1 Isothermal

2 Adiabatic

3 Isobaric

4 Isochoric

NEET - 2019

PHXI12:THERMODYNAMICS

371479 Assertion :
An adiabatic process is an isoentropic process.
Reason :
Change in entropy is zero in case of adiabatic process.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

In adiabatic process $Δ S = \frac{Δ Q}{T} = 0$ , since there is no heat exchange $(Δ Q = 0)$ (with the surroundings).
$\Rightarrow S =$ constant
So, this process is called isentropic
So correct option is (1).

PHXI12:THERMODYNAMICS

371480 Assertion :
Work done by a gas in isothermal expansion is more than the work done by the gas in the same expansion, adiabatically.
Reason :
Temperature remains constant in isothermal expansion and not in adiabatic expansion.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

Adiabatic $Δ Q = 0$
$\Rightarrow | Δ U | = | Δ W |$ (by first law of thermodynamics) Isothermal $Δ T = 0$
$\Rightarrow Δ Q = Δ W$
$\Rightarrow$ complete $Δ Q$ is used as work in isothermal.
$\Rightarrow$ work done in isothermal expansion is greater than in adiabatic expansion. However, the reason lacks precision, attributing the difference to temperature alone, while it's influenced by the change in internal energy. So correct option is (2).

PHXI12:THERMODYNAMICS

371481 $Δ U + Δ W = 0$ is valid for

1 Isothermal process

2 Adiabatic process

3 Isochoric process

4 Isobaric process

Explanation:

In adiabatic process
$\begin{aligned} Δ Q = 0 \Rightarrow Δ U + Δ W = 0 \\ (∵ Δ Q = Δ U + Δ W) \end{aligned}$

PHXI12:THERMODYNAMICS

371482 A tyre pumped to a pressure $3.375 atm$ at $27^{\circ} C$ suddenly bursts. What is the final temperature $(γ = 1.5)$ ?

1

- 27^{\circ} C

2

27^{\circ} C

3

- 73^{\circ} C

4

0^{\circ} C

Explanation:

Sudden bursting of a tyre can be treated as adiabatic expansion
$T_{1}^{γ} P_{1}^{1 - γ} = T_{2}^{γ} P_{2}^{1 - γ}$
${(\frac{T_{1}}{T_{2}})}^{γ} = {(\frac{P_{1}}{P_{2}})}^{γ - 1} \Rightarrow {(\frac{300}{T_{2}})}^{3 / 2} = {(\frac{3.375}{1})}^{3 / 2 - 1}$
$T_{2} = \frac{300}{{(3.375)}^{1 / 3}} = 200 K = - 73^{\circ} C$

PHXI12:THERMODYNAMICS

371478 In which of the following processes, heat is neither absorbed nor released by a system?

1 Isothermal

2 Adiabatic

3 Isobaric

4 Isochoric

NEET - 2019

PHXI12:THERMODYNAMICS

371479 Assertion :
An adiabatic process is an isoentropic process.
Reason :
Change in entropy is zero in case of adiabatic process.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

In adiabatic process $Δ S = \frac{Δ Q}{T} = 0$ , since there is no heat exchange $(Δ Q = 0)$ (with the surroundings).
$\Rightarrow S =$ constant
So, this process is called isentropic
So correct option is (1).

PHXI12:THERMODYNAMICS

371480 Assertion :
Work done by a gas in isothermal expansion is more than the work done by the gas in the same expansion, adiabatically.
Reason :
Temperature remains constant in isothermal expansion and not in adiabatic expansion.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

Adiabatic $Δ Q = 0$
$\Rightarrow | Δ U | = | Δ W |$ (by first law of thermodynamics) Isothermal $Δ T = 0$
$\Rightarrow Δ Q = Δ W$
$\Rightarrow$ complete $Δ Q$ is used as work in isothermal.
$\Rightarrow$ work done in isothermal expansion is greater than in adiabatic expansion. However, the reason lacks precision, attributing the difference to temperature alone, while it's influenced by the change in internal energy. So correct option is (2).

PHXI12:THERMODYNAMICS

371481 $Δ U + Δ W = 0$ is valid for

1 Isothermal process

2 Adiabatic process

3 Isochoric process

4 Isobaric process

Explanation:

In adiabatic process
$\begin{aligned} Δ Q = 0 \Rightarrow Δ U + Δ W = 0 \\ (∵ Δ Q = Δ U + Δ W) \end{aligned}$

PHXI12:THERMODYNAMICS

371482 A tyre pumped to a pressure $3.375 atm$ at $27^{\circ} C$ suddenly bursts. What is the final temperature $(γ = 1.5)$ ?

1

- 27^{\circ} C

2

27^{\circ} C

3

- 73^{\circ} C

4

0^{\circ} C

Explanation:

Sudden bursting of a tyre can be treated as adiabatic expansion
$T_{1}^{γ} P_{1}^{1 - γ} = T_{2}^{γ} P_{2}^{1 - γ}$
${(\frac{T_{1}}{T_{2}})}^{γ} = {(\frac{P_{1}}{P_{2}})}^{γ - 1} \Rightarrow {(\frac{300}{T_{2}})}^{3 / 2} = {(\frac{3.375}{1})}^{3 / 2 - 1}$
$T_{2} = \frac{300}{{(3.375)}^{1 / 3}} = 200 K = - 73^{\circ} C$

PHXI12:THERMODYNAMICS

371478 In which of the following processes, heat is neither absorbed nor released by a system?

1 Isothermal

2 Adiabatic

3 Isobaric

4 Isochoric

NEET - 2019

PHXI12:THERMODYNAMICS

371479 Assertion :
An adiabatic process is an isoentropic process.
Reason :
Change in entropy is zero in case of adiabatic process.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

In adiabatic process $Δ S = \frac{Δ Q}{T} = 0$ , since there is no heat exchange $(Δ Q = 0)$ (with the surroundings).
$\Rightarrow S =$ constant
So, this process is called isentropic
So correct option is (1).

PHXI12:THERMODYNAMICS

371480 Assertion :
Work done by a gas in isothermal expansion is more than the work done by the gas in the same expansion, adiabatically.
Reason :
Temperature remains constant in isothermal expansion and not in adiabatic expansion.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

Adiabatic $Δ Q = 0$
$\Rightarrow | Δ U | = | Δ W |$ (by first law of thermodynamics) Isothermal $Δ T = 0$
$\Rightarrow Δ Q = Δ W$
$\Rightarrow$ complete $Δ Q$ is used as work in isothermal.
$\Rightarrow$ work done in isothermal expansion is greater than in adiabatic expansion. However, the reason lacks precision, attributing the difference to temperature alone, while it's influenced by the change in internal energy. So correct option is (2).

PHXI12:THERMODYNAMICS

371481 $Δ U + Δ W = 0$ is valid for

1 Isothermal process

2 Adiabatic process

3 Isochoric process

4 Isobaric process

Explanation:

In adiabatic process
$\begin{aligned} Δ Q = 0 \Rightarrow Δ U + Δ W = 0 \\ (∵ Δ Q = Δ U + Δ W) \end{aligned}$

PHXI12:THERMODYNAMICS

371482 A tyre pumped to a pressure $3.375 atm$ at $27^{\circ} C$ suddenly bursts. What is the final temperature $(γ = 1.5)$ ?

1

- 27^{\circ} C

2

27^{\circ} C

3

- 73^{\circ} C

4

0^{\circ} C

Explanation:

Sudden bursting of a tyre can be treated as adiabatic expansion
$T_{1}^{γ} P_{1}^{1 - γ} = T_{2}^{γ} P_{2}^{1 - γ}$
${(\frac{T_{1}}{T_{2}})}^{γ} = {(\frac{P_{1}}{P_{2}})}^{γ - 1} \Rightarrow {(\frac{300}{T_{2}})}^{3 / 2} = {(\frac{3.375}{1})}^{3 / 2 - 1}$
$T_{2} = \frac{300}{{(3.375)}^{1 / 3}} = 200 K = - 73^{\circ} C$

PHXI12:THERMODYNAMICS

371478 In which of the following processes, heat is neither absorbed nor released by a system?

1 Isothermal

2 Adiabatic

3 Isobaric

4 Isochoric

NEET - 2019

PHXI12:THERMODYNAMICS

371479 Assertion :
An adiabatic process is an isoentropic process.
Reason :
Change in entropy is zero in case of adiabatic process.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

In adiabatic process $Δ S = \frac{Δ Q}{T} = 0$ , since there is no heat exchange $(Δ Q = 0)$ (with the surroundings).
$\Rightarrow S =$ constant
So, this process is called isentropic
So correct option is (1).

PHXI12:THERMODYNAMICS

371480 Assertion :
Work done by a gas in isothermal expansion is more than the work done by the gas in the same expansion, adiabatically.
Reason :
Temperature remains constant in isothermal expansion and not in adiabatic expansion.

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

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

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but reason is correct.

Explanation:

Adiabatic $Δ Q = 0$
$\Rightarrow | Δ U | = | Δ W |$ (by first law of thermodynamics) Isothermal $Δ T = 0$
$\Rightarrow Δ Q = Δ W$
$\Rightarrow$ complete $Δ Q$ is used as work in isothermal.
$\Rightarrow$ work done in isothermal expansion is greater than in adiabatic expansion. However, the reason lacks precision, attributing the difference to temperature alone, while it's influenced by the change in internal energy. So correct option is (2).

PHXI12:THERMODYNAMICS

371481 $Δ U + Δ W = 0$ is valid for

1 Isothermal process

2 Adiabatic process

3 Isochoric process

4 Isobaric process

Explanation:

In adiabatic process
$\begin{aligned} Δ Q = 0 \Rightarrow Δ U + Δ W = 0 \\ (∵ Δ Q = Δ U + Δ W) \end{aligned}$

PHXI12:THERMODYNAMICS

371482 A tyre pumped to a pressure $3.375 atm$ at $27^{\circ} C$ suddenly bursts. What is the final temperature $(γ = 1.5)$ ?

1

- 27^{\circ} C

2

27^{\circ} C

3

- 73^{\circ} C

4

0^{\circ} C

Explanation:

Sudden bursting of a tyre can be treated as adiabatic expansion
$T_{1}^{γ} P_{1}^{1 - γ} = T_{2}^{γ} P_{2}^{1 - γ}$
${(\frac{T_{1}}{T_{2}})}^{γ} = {(\frac{P_{1}}{P_{2}})}^{γ - 1} \Rightarrow {(\frac{300}{T_{2}})}^{3 / 2} = {(\frac{3.375}{1})}^{3 / 2 - 1}$
$T_{2} = \frac{300}{{(3.375)}^{1 / 3}} = 200 K = - 73^{\circ} C$