D Heat and work are path function internal energy is state function. From $1^{\text {st }}$ law of thermodynamics $\Delta \mathrm{Q}=\Delta \mathrm{W}+\Delta \mathrm{U}$ $\Delta \mathrm{U}=\Delta \mathrm{Q}-\Delta \mathrm{W}$ So, $\Delta \mathrm{Q}-\Delta \mathrm{W}$ is not a path function.
BCECE-2005
Thermodynamics
148307
If $\alpha$ is the coefficient of performance of a refrigerator and ' $Q_{1}$ ' is heat released to the hot reservoir, then the heat extracted from the cold reservoir ' $Q_{2}$ ' is
1 $\frac{\alpha Q_{1}}{\alpha-1}$
2 $\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
3 $\frac{1+\alpha}{\alpha} Q_{1}$
4 $\frac{\alpha-1}{\alpha} \mathrm{Q}_{1}$
Explanation:
B Coefficient of performance (COP) of a refrigerator, $\alpha=\frac{\mathrm{Q}_{2}}{\mathrm{Q}_{1}-\mathrm{Q}_{2}}$ $\frac{1}{\alpha}=\frac{\mathrm{Q}_{1}-\mathrm{Q}_{2}}{\mathrm{Q}_{2}}=\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}-1$ $\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}=\frac{1}{\alpha}+1$ $\mathrm{Q}_{2}=\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
MHT-CET 2009
Thermodynamics
148313
Which of the following statement is true?
1 Internal energy of a gas depends only on the state of the gas.
2 In an isothermal process change in internal energy is maximum.
3 Area under pressure, volume graph equals heat supplied in any process.
4 Work done is state dependent but not path dependent.
Explanation:
A In taking a system from one state to another by different processes, the heat transferred $Q$ and work done $\mathrm{W}$ are different, but their $\mathrm{Q}-\mathrm{W}$ is same for all processes. It gives the internal energy of the system. $\Delta \mathrm{U}=\mathrm{Q}-\mathrm{W}$ Thus, internal energy $U$ of a thermodynamic system is a characteristic property of the state of the system, it does not matter how that state has been obtained.
J and K CET- 2006
Thermodynamics
148320
Which of the following statements (s) is/are true? "Internal energy of an ideal gas....."
1 decreases in an isothermal process
2 remains constant in an isothermal process
3 increases in an isobaric process
4 decreases in an isobaric expansion
Explanation:
B Internal energy of an ideal gas depends upon the temperature of gas. In isothermal process $\Delta \mathrm{U}=0$ In isobaric expansion $\mathrm{V} \propto \mathrm{T}$ So $\Delta \mathrm{U}$ increases. Hence, internal energy of an ideal gas remains constant in an isothermal process.
WB JEE 2018
Thermodynamics
148322
An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is
1 $3 / 8$
2 $3 / 5$
3 $3 / 4$
4 $2 / 5$
Explanation:
B Fraction $=\frac{\Delta U}{\Delta Q}=\frac{C_{v}}{C_{p}}$ We know that, $\gamma=\frac{\mathrm{C}_{\mathrm{p}}}{\mathrm{C}_{\mathrm{v}}}$ For monatomic gas, $\gamma=\frac{5}{3}$ So, $\quad \frac{\mathrm{C}_{\mathrm{v}}}{\mathrm{C}_{\mathrm{p}}}=\frac{1}{\gamma}=\frac{3}{5}$
D Heat and work are path function internal energy is state function. From $1^{\text {st }}$ law of thermodynamics $\Delta \mathrm{Q}=\Delta \mathrm{W}+\Delta \mathrm{U}$ $\Delta \mathrm{U}=\Delta \mathrm{Q}-\Delta \mathrm{W}$ So, $\Delta \mathrm{Q}-\Delta \mathrm{W}$ is not a path function.
BCECE-2005
Thermodynamics
148307
If $\alpha$ is the coefficient of performance of a refrigerator and ' $Q_{1}$ ' is heat released to the hot reservoir, then the heat extracted from the cold reservoir ' $Q_{2}$ ' is
1 $\frac{\alpha Q_{1}}{\alpha-1}$
2 $\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
3 $\frac{1+\alpha}{\alpha} Q_{1}$
4 $\frac{\alpha-1}{\alpha} \mathrm{Q}_{1}$
Explanation:
B Coefficient of performance (COP) of a refrigerator, $\alpha=\frac{\mathrm{Q}_{2}}{\mathrm{Q}_{1}-\mathrm{Q}_{2}}$ $\frac{1}{\alpha}=\frac{\mathrm{Q}_{1}-\mathrm{Q}_{2}}{\mathrm{Q}_{2}}=\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}-1$ $\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}=\frac{1}{\alpha}+1$ $\mathrm{Q}_{2}=\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
MHT-CET 2009
Thermodynamics
148313
Which of the following statement is true?
1 Internal energy of a gas depends only on the state of the gas.
2 In an isothermal process change in internal energy is maximum.
3 Area under pressure, volume graph equals heat supplied in any process.
4 Work done is state dependent but not path dependent.
Explanation:
A In taking a system from one state to another by different processes, the heat transferred $Q$ and work done $\mathrm{W}$ are different, but their $\mathrm{Q}-\mathrm{W}$ is same for all processes. It gives the internal energy of the system. $\Delta \mathrm{U}=\mathrm{Q}-\mathrm{W}$ Thus, internal energy $U$ of a thermodynamic system is a characteristic property of the state of the system, it does not matter how that state has been obtained.
J and K CET- 2006
Thermodynamics
148320
Which of the following statements (s) is/are true? "Internal energy of an ideal gas....."
1 decreases in an isothermal process
2 remains constant in an isothermal process
3 increases in an isobaric process
4 decreases in an isobaric expansion
Explanation:
B Internal energy of an ideal gas depends upon the temperature of gas. In isothermal process $\Delta \mathrm{U}=0$ In isobaric expansion $\mathrm{V} \propto \mathrm{T}$ So $\Delta \mathrm{U}$ increases. Hence, internal energy of an ideal gas remains constant in an isothermal process.
WB JEE 2018
Thermodynamics
148322
An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is
1 $3 / 8$
2 $3 / 5$
3 $3 / 4$
4 $2 / 5$
Explanation:
B Fraction $=\frac{\Delta U}{\Delta Q}=\frac{C_{v}}{C_{p}}$ We know that, $\gamma=\frac{\mathrm{C}_{\mathrm{p}}}{\mathrm{C}_{\mathrm{v}}}$ For monatomic gas, $\gamma=\frac{5}{3}$ So, $\quad \frac{\mathrm{C}_{\mathrm{v}}}{\mathrm{C}_{\mathrm{p}}}=\frac{1}{\gamma}=\frac{3}{5}$
D Heat and work are path function internal energy is state function. From $1^{\text {st }}$ law of thermodynamics $\Delta \mathrm{Q}=\Delta \mathrm{W}+\Delta \mathrm{U}$ $\Delta \mathrm{U}=\Delta \mathrm{Q}-\Delta \mathrm{W}$ So, $\Delta \mathrm{Q}-\Delta \mathrm{W}$ is not a path function.
BCECE-2005
Thermodynamics
148307
If $\alpha$ is the coefficient of performance of a refrigerator and ' $Q_{1}$ ' is heat released to the hot reservoir, then the heat extracted from the cold reservoir ' $Q_{2}$ ' is
1 $\frac{\alpha Q_{1}}{\alpha-1}$
2 $\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
3 $\frac{1+\alpha}{\alpha} Q_{1}$
4 $\frac{\alpha-1}{\alpha} \mathrm{Q}_{1}$
Explanation:
B Coefficient of performance (COP) of a refrigerator, $\alpha=\frac{\mathrm{Q}_{2}}{\mathrm{Q}_{1}-\mathrm{Q}_{2}}$ $\frac{1}{\alpha}=\frac{\mathrm{Q}_{1}-\mathrm{Q}_{2}}{\mathrm{Q}_{2}}=\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}-1$ $\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}=\frac{1}{\alpha}+1$ $\mathrm{Q}_{2}=\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
MHT-CET 2009
Thermodynamics
148313
Which of the following statement is true?
1 Internal energy of a gas depends only on the state of the gas.
2 In an isothermal process change in internal energy is maximum.
3 Area under pressure, volume graph equals heat supplied in any process.
4 Work done is state dependent but not path dependent.
Explanation:
A In taking a system from one state to another by different processes, the heat transferred $Q$ and work done $\mathrm{W}$ are different, but their $\mathrm{Q}-\mathrm{W}$ is same for all processes. It gives the internal energy of the system. $\Delta \mathrm{U}=\mathrm{Q}-\mathrm{W}$ Thus, internal energy $U$ of a thermodynamic system is a characteristic property of the state of the system, it does not matter how that state has been obtained.
J and K CET- 2006
Thermodynamics
148320
Which of the following statements (s) is/are true? "Internal energy of an ideal gas....."
1 decreases in an isothermal process
2 remains constant in an isothermal process
3 increases in an isobaric process
4 decreases in an isobaric expansion
Explanation:
B Internal energy of an ideal gas depends upon the temperature of gas. In isothermal process $\Delta \mathrm{U}=0$ In isobaric expansion $\mathrm{V} \propto \mathrm{T}$ So $\Delta \mathrm{U}$ increases. Hence, internal energy of an ideal gas remains constant in an isothermal process.
WB JEE 2018
Thermodynamics
148322
An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is
1 $3 / 8$
2 $3 / 5$
3 $3 / 4$
4 $2 / 5$
Explanation:
B Fraction $=\frac{\Delta U}{\Delta Q}=\frac{C_{v}}{C_{p}}$ We know that, $\gamma=\frac{\mathrm{C}_{\mathrm{p}}}{\mathrm{C}_{\mathrm{v}}}$ For monatomic gas, $\gamma=\frac{5}{3}$ So, $\quad \frac{\mathrm{C}_{\mathrm{v}}}{\mathrm{C}_{\mathrm{p}}}=\frac{1}{\gamma}=\frac{3}{5}$
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
Thermodynamics
148304
Which is not a path function?
1 $\Delta \mathrm{Q}$
2 $\Delta \mathrm{Q}+\Delta \mathrm{W}$
3 $\Delta \mathrm{W}$
4 $\Delta \mathrm{Q}-\Delta \mathrm{W}$
Explanation:
D Heat and work are path function internal energy is state function. From $1^{\text {st }}$ law of thermodynamics $\Delta \mathrm{Q}=\Delta \mathrm{W}+\Delta \mathrm{U}$ $\Delta \mathrm{U}=\Delta \mathrm{Q}-\Delta \mathrm{W}$ So, $\Delta \mathrm{Q}-\Delta \mathrm{W}$ is not a path function.
BCECE-2005
Thermodynamics
148307
If $\alpha$ is the coefficient of performance of a refrigerator and ' $Q_{1}$ ' is heat released to the hot reservoir, then the heat extracted from the cold reservoir ' $Q_{2}$ ' is
1 $\frac{\alpha Q_{1}}{\alpha-1}$
2 $\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
3 $\frac{1+\alpha}{\alpha} Q_{1}$
4 $\frac{\alpha-1}{\alpha} \mathrm{Q}_{1}$
Explanation:
B Coefficient of performance (COP) of a refrigerator, $\alpha=\frac{\mathrm{Q}_{2}}{\mathrm{Q}_{1}-\mathrm{Q}_{2}}$ $\frac{1}{\alpha}=\frac{\mathrm{Q}_{1}-\mathrm{Q}_{2}}{\mathrm{Q}_{2}}=\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}-1$ $\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}=\frac{1}{\alpha}+1$ $\mathrm{Q}_{2}=\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
MHT-CET 2009
Thermodynamics
148313
Which of the following statement is true?
1 Internal energy of a gas depends only on the state of the gas.
2 In an isothermal process change in internal energy is maximum.
3 Area under pressure, volume graph equals heat supplied in any process.
4 Work done is state dependent but not path dependent.
Explanation:
A In taking a system from one state to another by different processes, the heat transferred $Q$ and work done $\mathrm{W}$ are different, but their $\mathrm{Q}-\mathrm{W}$ is same for all processes. It gives the internal energy of the system. $\Delta \mathrm{U}=\mathrm{Q}-\mathrm{W}$ Thus, internal energy $U$ of a thermodynamic system is a characteristic property of the state of the system, it does not matter how that state has been obtained.
J and K CET- 2006
Thermodynamics
148320
Which of the following statements (s) is/are true? "Internal energy of an ideal gas....."
1 decreases in an isothermal process
2 remains constant in an isothermal process
3 increases in an isobaric process
4 decreases in an isobaric expansion
Explanation:
B Internal energy of an ideal gas depends upon the temperature of gas. In isothermal process $\Delta \mathrm{U}=0$ In isobaric expansion $\mathrm{V} \propto \mathrm{T}$ So $\Delta \mathrm{U}$ increases. Hence, internal energy of an ideal gas remains constant in an isothermal process.
WB JEE 2018
Thermodynamics
148322
An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is
1 $3 / 8$
2 $3 / 5$
3 $3 / 4$
4 $2 / 5$
Explanation:
B Fraction $=\frac{\Delta U}{\Delta Q}=\frac{C_{v}}{C_{p}}$ We know that, $\gamma=\frac{\mathrm{C}_{\mathrm{p}}}{\mathrm{C}_{\mathrm{v}}}$ For monatomic gas, $\gamma=\frac{5}{3}$ So, $\quad \frac{\mathrm{C}_{\mathrm{v}}}{\mathrm{C}_{\mathrm{p}}}=\frac{1}{\gamma}=\frac{3}{5}$
D Heat and work are path function internal energy is state function. From $1^{\text {st }}$ law of thermodynamics $\Delta \mathrm{Q}=\Delta \mathrm{W}+\Delta \mathrm{U}$ $\Delta \mathrm{U}=\Delta \mathrm{Q}-\Delta \mathrm{W}$ So, $\Delta \mathrm{Q}-\Delta \mathrm{W}$ is not a path function.
BCECE-2005
Thermodynamics
148307
If $\alpha$ is the coefficient of performance of a refrigerator and ' $Q_{1}$ ' is heat released to the hot reservoir, then the heat extracted from the cold reservoir ' $Q_{2}$ ' is
1 $\frac{\alpha Q_{1}}{\alpha-1}$
2 $\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
3 $\frac{1+\alpha}{\alpha} Q_{1}$
4 $\frac{\alpha-1}{\alpha} \mathrm{Q}_{1}$
Explanation:
B Coefficient of performance (COP) of a refrigerator, $\alpha=\frac{\mathrm{Q}_{2}}{\mathrm{Q}_{1}-\mathrm{Q}_{2}}$ $\frac{1}{\alpha}=\frac{\mathrm{Q}_{1}-\mathrm{Q}_{2}}{\mathrm{Q}_{2}}=\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}-1$ $\frac{\mathrm{Q}_{1}}{\mathrm{Q}_{2}}=\frac{1}{\alpha}+1$ $\mathrm{Q}_{2}=\frac{\alpha \mathrm{Q}_{1}}{1+\alpha}$
MHT-CET 2009
Thermodynamics
148313
Which of the following statement is true?
1 Internal energy of a gas depends only on the state of the gas.
2 In an isothermal process change in internal energy is maximum.
3 Area under pressure, volume graph equals heat supplied in any process.
4 Work done is state dependent but not path dependent.
Explanation:
A In taking a system from one state to another by different processes, the heat transferred $Q$ and work done $\mathrm{W}$ are different, but their $\mathrm{Q}-\mathrm{W}$ is same for all processes. It gives the internal energy of the system. $\Delta \mathrm{U}=\mathrm{Q}-\mathrm{W}$ Thus, internal energy $U$ of a thermodynamic system is a characteristic property of the state of the system, it does not matter how that state has been obtained.
J and K CET- 2006
Thermodynamics
148320
Which of the following statements (s) is/are true? "Internal energy of an ideal gas....."
1 decreases in an isothermal process
2 remains constant in an isothermal process
3 increases in an isobaric process
4 decreases in an isobaric expansion
Explanation:
B Internal energy of an ideal gas depends upon the temperature of gas. In isothermal process $\Delta \mathrm{U}=0$ In isobaric expansion $\mathrm{V} \propto \mathrm{T}$ So $\Delta \mathrm{U}$ increases. Hence, internal energy of an ideal gas remains constant in an isothermal process.
WB JEE 2018
Thermodynamics
148322
An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy of the gas is
1 $3 / 8$
2 $3 / 5$
3 $3 / 4$
4 $2 / 5$
Explanation:
B Fraction $=\frac{\Delta U}{\Delta Q}=\frac{C_{v}}{C_{p}}$ We know that, $\gamma=\frac{\mathrm{C}_{\mathrm{p}}}{\mathrm{C}_{\mathrm{v}}}$ For monatomic gas, $\gamma=\frac{5}{3}$ So, $\quad \frac{\mathrm{C}_{\mathrm{v}}}{\mathrm{C}_{\mathrm{p}}}=\frac{1}{\gamma}=\frac{3}{5}$