For an isochoric process, \(\mathrm{\Delta \mathrm{V}=0}\) In this process, the first law of thermodynamics \(\rm{ \mathrm{q}=\Delta \mathrm{U}-\mathrm{W} \\ \mathrm{q}=\Delta \mathrm{U}-\mathrm{p} \Delta \mathrm{V} \\ \text { As } \Delta \mathrm{V}=0 \\ \mathrm{q}_{\mathrm{v}}=\Delta \mathrm{U}}\)
MHTCET - 2016
CHXI06:THERMODYNAMICS
369335
When \({\text{x kJ}}\) heat is provided to a system, work equivalent to \(\mathrm{yJ}\) is done on it. What is internal energy change during this operation?
1 \((1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
2 \({\text{1000(x + y) J}}\)
3 \({\text{(x + 1000 y) J}}\)
4 \({\text{x + yJ}}\)
Explanation:
\({\text{Q =+ x k J = 1000 x J, W = +y J}}\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=(1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369336
When 1 mole of gas is heated at constant volume, the temperature rises from \(273 \mathrm{~K}\) to \(546 \mathrm{~K}\). If heat supplied to the gas is \(\mathrm{xJ}\), then find the correct statement from the following.
At constant volume, \(\Delta \mathrm{V}=0\) Workdone, \(\mathrm{W}=-\mathrm{P} \Delta \mathrm{V}=0\) According to first law of thermodynamics \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(\therefore \Delta \mathrm{U}=\mathrm{Q}=\mathrm{x} \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369337
In a process, a system performs \(238 \mathrm{~J}\) of work on it's surrounding by absorbing \(54 \mathrm{~J}\) of heat. What is the change in internal energy of system during this operation?
1 \(222 \mathrm{~J}\)
2 \(-192 \mathrm{~J}\)
3 \(54 \mathrm{~J}\)
4 \(-184 \mathrm{~J}\)
Explanation:
\(\mathrm{W}=-238 \mathrm{~J}\) (workdone by the system), \(\mathrm{Q}=54 \mathrm{~J}\) (heat absorbed \()\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=54-238=-184 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369338
Assertion : First law of thermodynamics is identical to the law of conservation of energy. Reason : It states that the total energy of the universe is constant.
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:
The first law of thermodynamics and the law of conservation of energy are equivalent, stating that the total energy in an isolated system remains constant, undergoing only transformations or transfers between the system and its surroundings. Thus, option (1) is correct.
For an isochoric process, \(\mathrm{\Delta \mathrm{V}=0}\) In this process, the first law of thermodynamics \(\rm{ \mathrm{q}=\Delta \mathrm{U}-\mathrm{W} \\ \mathrm{q}=\Delta \mathrm{U}-\mathrm{p} \Delta \mathrm{V} \\ \text { As } \Delta \mathrm{V}=0 \\ \mathrm{q}_{\mathrm{v}}=\Delta \mathrm{U}}\)
MHTCET - 2016
CHXI06:THERMODYNAMICS
369335
When \({\text{x kJ}}\) heat is provided to a system, work equivalent to \(\mathrm{yJ}\) is done on it. What is internal energy change during this operation?
1 \((1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
2 \({\text{1000(x + y) J}}\)
3 \({\text{(x + 1000 y) J}}\)
4 \({\text{x + yJ}}\)
Explanation:
\({\text{Q =+ x k J = 1000 x J, W = +y J}}\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=(1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369336
When 1 mole of gas is heated at constant volume, the temperature rises from \(273 \mathrm{~K}\) to \(546 \mathrm{~K}\). If heat supplied to the gas is \(\mathrm{xJ}\), then find the correct statement from the following.
At constant volume, \(\Delta \mathrm{V}=0\) Workdone, \(\mathrm{W}=-\mathrm{P} \Delta \mathrm{V}=0\) According to first law of thermodynamics \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(\therefore \Delta \mathrm{U}=\mathrm{Q}=\mathrm{x} \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369337
In a process, a system performs \(238 \mathrm{~J}\) of work on it's surrounding by absorbing \(54 \mathrm{~J}\) of heat. What is the change in internal energy of system during this operation?
1 \(222 \mathrm{~J}\)
2 \(-192 \mathrm{~J}\)
3 \(54 \mathrm{~J}\)
4 \(-184 \mathrm{~J}\)
Explanation:
\(\mathrm{W}=-238 \mathrm{~J}\) (workdone by the system), \(\mathrm{Q}=54 \mathrm{~J}\) (heat absorbed \()\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=54-238=-184 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369338
Assertion : First law of thermodynamics is identical to the law of conservation of energy. Reason : It states that the total energy of the universe is constant.
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:
The first law of thermodynamics and the law of conservation of energy are equivalent, stating that the total energy in an isolated system remains constant, undergoing only transformations or transfers between the system and its surroundings. Thus, option (1) is correct.
For an isochoric process, \(\mathrm{\Delta \mathrm{V}=0}\) In this process, the first law of thermodynamics \(\rm{ \mathrm{q}=\Delta \mathrm{U}-\mathrm{W} \\ \mathrm{q}=\Delta \mathrm{U}-\mathrm{p} \Delta \mathrm{V} \\ \text { As } \Delta \mathrm{V}=0 \\ \mathrm{q}_{\mathrm{v}}=\Delta \mathrm{U}}\)
MHTCET - 2016
CHXI06:THERMODYNAMICS
369335
When \({\text{x kJ}}\) heat is provided to a system, work equivalent to \(\mathrm{yJ}\) is done on it. What is internal energy change during this operation?
1 \((1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
2 \({\text{1000(x + y) J}}\)
3 \({\text{(x + 1000 y) J}}\)
4 \({\text{x + yJ}}\)
Explanation:
\({\text{Q =+ x k J = 1000 x J, W = +y J}}\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=(1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369336
When 1 mole of gas is heated at constant volume, the temperature rises from \(273 \mathrm{~K}\) to \(546 \mathrm{~K}\). If heat supplied to the gas is \(\mathrm{xJ}\), then find the correct statement from the following.
At constant volume, \(\Delta \mathrm{V}=0\) Workdone, \(\mathrm{W}=-\mathrm{P} \Delta \mathrm{V}=0\) According to first law of thermodynamics \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(\therefore \Delta \mathrm{U}=\mathrm{Q}=\mathrm{x} \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369337
In a process, a system performs \(238 \mathrm{~J}\) of work on it's surrounding by absorbing \(54 \mathrm{~J}\) of heat. What is the change in internal energy of system during this operation?
1 \(222 \mathrm{~J}\)
2 \(-192 \mathrm{~J}\)
3 \(54 \mathrm{~J}\)
4 \(-184 \mathrm{~J}\)
Explanation:
\(\mathrm{W}=-238 \mathrm{~J}\) (workdone by the system), \(\mathrm{Q}=54 \mathrm{~J}\) (heat absorbed \()\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=54-238=-184 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369338
Assertion : First law of thermodynamics is identical to the law of conservation of energy. Reason : It states that the total energy of the universe is constant.
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:
The first law of thermodynamics and the law of conservation of energy are equivalent, stating that the total energy in an isolated system remains constant, undergoing only transformations or transfers between the system and its surroundings. Thus, option (1) is correct.
For an isochoric process, \(\mathrm{\Delta \mathrm{V}=0}\) In this process, the first law of thermodynamics \(\rm{ \mathrm{q}=\Delta \mathrm{U}-\mathrm{W} \\ \mathrm{q}=\Delta \mathrm{U}-\mathrm{p} \Delta \mathrm{V} \\ \text { As } \Delta \mathrm{V}=0 \\ \mathrm{q}_{\mathrm{v}}=\Delta \mathrm{U}}\)
MHTCET - 2016
CHXI06:THERMODYNAMICS
369335
When \({\text{x kJ}}\) heat is provided to a system, work equivalent to \(\mathrm{yJ}\) is done on it. What is internal energy change during this operation?
1 \((1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
2 \({\text{1000(x + y) J}}\)
3 \({\text{(x + 1000 y) J}}\)
4 \({\text{x + yJ}}\)
Explanation:
\({\text{Q =+ x k J = 1000 x J, W = +y J}}\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=(1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369336
When 1 mole of gas is heated at constant volume, the temperature rises from \(273 \mathrm{~K}\) to \(546 \mathrm{~K}\). If heat supplied to the gas is \(\mathrm{xJ}\), then find the correct statement from the following.
At constant volume, \(\Delta \mathrm{V}=0\) Workdone, \(\mathrm{W}=-\mathrm{P} \Delta \mathrm{V}=0\) According to first law of thermodynamics \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(\therefore \Delta \mathrm{U}=\mathrm{Q}=\mathrm{x} \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369337
In a process, a system performs \(238 \mathrm{~J}\) of work on it's surrounding by absorbing \(54 \mathrm{~J}\) of heat. What is the change in internal energy of system during this operation?
1 \(222 \mathrm{~J}\)
2 \(-192 \mathrm{~J}\)
3 \(54 \mathrm{~J}\)
4 \(-184 \mathrm{~J}\)
Explanation:
\(\mathrm{W}=-238 \mathrm{~J}\) (workdone by the system), \(\mathrm{Q}=54 \mathrm{~J}\) (heat absorbed \()\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=54-238=-184 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369338
Assertion : First law of thermodynamics is identical to the law of conservation of energy. Reason : It states that the total energy of the universe is constant.
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:
The first law of thermodynamics and the law of conservation of energy are equivalent, stating that the total energy in an isolated system remains constant, undergoing only transformations or transfers between the system and its surroundings. Thus, option (1) is correct.
For an isochoric process, \(\mathrm{\Delta \mathrm{V}=0}\) In this process, the first law of thermodynamics \(\rm{ \mathrm{q}=\Delta \mathrm{U}-\mathrm{W} \\ \mathrm{q}=\Delta \mathrm{U}-\mathrm{p} \Delta \mathrm{V} \\ \text { As } \Delta \mathrm{V}=0 \\ \mathrm{q}_{\mathrm{v}}=\Delta \mathrm{U}}\)
MHTCET - 2016
CHXI06:THERMODYNAMICS
369335
When \({\text{x kJ}}\) heat is provided to a system, work equivalent to \(\mathrm{yJ}\) is done on it. What is internal energy change during this operation?
1 \((1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
2 \({\text{1000(x + y) J}}\)
3 \({\text{(x + 1000 y) J}}\)
4 \({\text{x + yJ}}\)
Explanation:
\({\text{Q =+ x k J = 1000 x J, W = +y J}}\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=(1000 \mathrm{x}+\mathrm{y}) \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369336
When 1 mole of gas is heated at constant volume, the temperature rises from \(273 \mathrm{~K}\) to \(546 \mathrm{~K}\). If heat supplied to the gas is \(\mathrm{xJ}\), then find the correct statement from the following.
At constant volume, \(\Delta \mathrm{V}=0\) Workdone, \(\mathrm{W}=-\mathrm{P} \Delta \mathrm{V}=0\) According to first law of thermodynamics \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(\therefore \Delta \mathrm{U}=\mathrm{Q}=\mathrm{x} \mathrm{J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369337
In a process, a system performs \(238 \mathrm{~J}\) of work on it's surrounding by absorbing \(54 \mathrm{~J}\) of heat. What is the change in internal energy of system during this operation?
1 \(222 \mathrm{~J}\)
2 \(-192 \mathrm{~J}\)
3 \(54 \mathrm{~J}\)
4 \(-184 \mathrm{~J}\)
Explanation:
\(\mathrm{W}=-238 \mathrm{~J}\) (workdone by the system), \(\mathrm{Q}=54 \mathrm{~J}\) (heat absorbed \()\) According to first law of thermodynamics, \(\Delta \mathrm{U}=\mathrm{Q}+\mathrm{W}\) \(=54-238=-184 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369338
Assertion : First law of thermodynamics is identical to the law of conservation of energy. Reason : It states that the total energy of the universe is constant.
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:
The first law of thermodynamics and the law of conservation of energy are equivalent, stating that the total energy in an isolated system remains constant, undergoing only transformations or transfers between the system and its surroundings. Thus, option (1) is correct.
