369146
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. The conditions are
1 High Temperature, High Pressure
2 Constant Temperature, Constant Pressure
3 Low Temperature, Low Pressure
4 Constant Volume, Constant Pressure
Explanation:
By first law of thermodynamics: \(\mathrm{q=\Delta U+(-w)}\) \(\mathrm{(-w)=p \Delta V}\) \(\mathrm{\therefore q=\Delta U+p \Delta V}\) \(\mathrm{\Delta V=0}\), since volume is constant. \(\mathrm{\therefore q_{v}=\Delta U+0}\) \(\mathrm{\Rightarrow q_{v}=\Delta U=}\) change in internal energy At constant pressure \(\mathrm{q_{p}=\Delta U+p \Delta V}\) But, \(\mathrm{\Delta U+p \Delta V=\Delta H}\) \(\mathrm{\therefore q_{p}=\Delta H=}\) change in enthalpy So, at constant volume and at constant pressure heat change is a state function because it is equal to change in internal energy and change in enthalpy respectively which are state functions.
CHXI06:THERMODYNAMICS
369147
Identify the state function among the following:
1 \(\mathrm{q}\)
2 \(\mathrm{q-w}\)
3 \(\mathrm{\dfrac{q}{w}}\)
4 \(\mathrm{q+w}\)
Explanation:
\(\mathrm{q+w=\Delta U}\) is a state function.
CHXI06:THERMODYNAMICS
369148
Which of the following are not state functions? (I) \(\mathrm{q+w}\) (II) \(\mathrm{q}\) (III) w (IV) H-TS
1 (I) and (IV)
2 (II), (III) and (IV)
3 (I), (II) and (III)
4 (II) and (III)
Explanation:
We know that heat (q) and work (w) are not state functions but \(\mathrm{(\mathrm{q}+\mathrm{w})}\) is a state function. \({\rm{H - TS}}\) (i.e. G) is also a state function.
CHXI06:THERMODYNAMICS
369149
Statement A : T, P and V are state variables or state functions. Statement B : Their values depend on the state of the system and not on how it is reached.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Values of state functions depend only on the state of the system and not on how it is reached.
CHXI06:THERMODYNAMICS
369150
In a change from state \(\mathrm{A}\) to state \(\mathrm{B}\) :
1 " \({\text{q}}\)" depends only on the initial and final states.
2 "\({\text{W}}\)" depends only on the initial and final states.
3 \(\Delta \mathrm{E}\) depends only on the initial and final states.
4 \(\Delta\)\({\text{E}}\) depends upon the path adopted by " \({\text{A}}\) " to change into " \({\text{B}}\) "
Explanation:
Because \(\Delta \mathrm{E}\) is a state function. Heat and work are path functions.
369146
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. The conditions are
1 High Temperature, High Pressure
2 Constant Temperature, Constant Pressure
3 Low Temperature, Low Pressure
4 Constant Volume, Constant Pressure
Explanation:
By first law of thermodynamics: \(\mathrm{q=\Delta U+(-w)}\) \(\mathrm{(-w)=p \Delta V}\) \(\mathrm{\therefore q=\Delta U+p \Delta V}\) \(\mathrm{\Delta V=0}\), since volume is constant. \(\mathrm{\therefore q_{v}=\Delta U+0}\) \(\mathrm{\Rightarrow q_{v}=\Delta U=}\) change in internal energy At constant pressure \(\mathrm{q_{p}=\Delta U+p \Delta V}\) But, \(\mathrm{\Delta U+p \Delta V=\Delta H}\) \(\mathrm{\therefore q_{p}=\Delta H=}\) change in enthalpy So, at constant volume and at constant pressure heat change is a state function because it is equal to change in internal energy and change in enthalpy respectively which are state functions.
CHXI06:THERMODYNAMICS
369147
Identify the state function among the following:
1 \(\mathrm{q}\)
2 \(\mathrm{q-w}\)
3 \(\mathrm{\dfrac{q}{w}}\)
4 \(\mathrm{q+w}\)
Explanation:
\(\mathrm{q+w=\Delta U}\) is a state function.
CHXI06:THERMODYNAMICS
369148
Which of the following are not state functions? (I) \(\mathrm{q+w}\) (II) \(\mathrm{q}\) (III) w (IV) H-TS
1 (I) and (IV)
2 (II), (III) and (IV)
3 (I), (II) and (III)
4 (II) and (III)
Explanation:
We know that heat (q) and work (w) are not state functions but \(\mathrm{(\mathrm{q}+\mathrm{w})}\) is a state function. \({\rm{H - TS}}\) (i.e. G) is also a state function.
CHXI06:THERMODYNAMICS
369149
Statement A : T, P and V are state variables or state functions. Statement B : Their values depend on the state of the system and not on how it is reached.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Values of state functions depend only on the state of the system and not on how it is reached.
CHXI06:THERMODYNAMICS
369150
In a change from state \(\mathrm{A}\) to state \(\mathrm{B}\) :
1 " \({\text{q}}\)" depends only on the initial and final states.
2 "\({\text{W}}\)" depends only on the initial and final states.
3 \(\Delta \mathrm{E}\) depends only on the initial and final states.
4 \(\Delta\)\({\text{E}}\) depends upon the path adopted by " \({\text{A}}\) " to change into " \({\text{B}}\) "
Explanation:
Because \(\Delta \mathrm{E}\) is a state function. Heat and work are path functions.
369146
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. The conditions are
1 High Temperature, High Pressure
2 Constant Temperature, Constant Pressure
3 Low Temperature, Low Pressure
4 Constant Volume, Constant Pressure
Explanation:
By first law of thermodynamics: \(\mathrm{q=\Delta U+(-w)}\) \(\mathrm{(-w)=p \Delta V}\) \(\mathrm{\therefore q=\Delta U+p \Delta V}\) \(\mathrm{\Delta V=0}\), since volume is constant. \(\mathrm{\therefore q_{v}=\Delta U+0}\) \(\mathrm{\Rightarrow q_{v}=\Delta U=}\) change in internal energy At constant pressure \(\mathrm{q_{p}=\Delta U+p \Delta V}\) But, \(\mathrm{\Delta U+p \Delta V=\Delta H}\) \(\mathrm{\therefore q_{p}=\Delta H=}\) change in enthalpy So, at constant volume and at constant pressure heat change is a state function because it is equal to change in internal energy and change in enthalpy respectively which are state functions.
CHXI06:THERMODYNAMICS
369147
Identify the state function among the following:
1 \(\mathrm{q}\)
2 \(\mathrm{q-w}\)
3 \(\mathrm{\dfrac{q}{w}}\)
4 \(\mathrm{q+w}\)
Explanation:
\(\mathrm{q+w=\Delta U}\) is a state function.
CHXI06:THERMODYNAMICS
369148
Which of the following are not state functions? (I) \(\mathrm{q+w}\) (II) \(\mathrm{q}\) (III) w (IV) H-TS
1 (I) and (IV)
2 (II), (III) and (IV)
3 (I), (II) and (III)
4 (II) and (III)
Explanation:
We know that heat (q) and work (w) are not state functions but \(\mathrm{(\mathrm{q}+\mathrm{w})}\) is a state function. \({\rm{H - TS}}\) (i.e. G) is also a state function.
CHXI06:THERMODYNAMICS
369149
Statement A : T, P and V are state variables or state functions. Statement B : Their values depend on the state of the system and not on how it is reached.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Values of state functions depend only on the state of the system and not on how it is reached.
CHXI06:THERMODYNAMICS
369150
In a change from state \(\mathrm{A}\) to state \(\mathrm{B}\) :
1 " \({\text{q}}\)" depends only on the initial and final states.
2 "\({\text{W}}\)" depends only on the initial and final states.
3 \(\Delta \mathrm{E}\) depends only on the initial and final states.
4 \(\Delta\)\({\text{E}}\) depends upon the path adopted by " \({\text{A}}\) " to change into " \({\text{B}}\) "
Explanation:
Because \(\Delta \mathrm{E}\) is a state function. Heat and work are path functions.
369146
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. The conditions are
1 High Temperature, High Pressure
2 Constant Temperature, Constant Pressure
3 Low Temperature, Low Pressure
4 Constant Volume, Constant Pressure
Explanation:
By first law of thermodynamics: \(\mathrm{q=\Delta U+(-w)}\) \(\mathrm{(-w)=p \Delta V}\) \(\mathrm{\therefore q=\Delta U+p \Delta V}\) \(\mathrm{\Delta V=0}\), since volume is constant. \(\mathrm{\therefore q_{v}=\Delta U+0}\) \(\mathrm{\Rightarrow q_{v}=\Delta U=}\) change in internal energy At constant pressure \(\mathrm{q_{p}=\Delta U+p \Delta V}\) But, \(\mathrm{\Delta U+p \Delta V=\Delta H}\) \(\mathrm{\therefore q_{p}=\Delta H=}\) change in enthalpy So, at constant volume and at constant pressure heat change is a state function because it is equal to change in internal energy and change in enthalpy respectively which are state functions.
CHXI06:THERMODYNAMICS
369147
Identify the state function among the following:
1 \(\mathrm{q}\)
2 \(\mathrm{q-w}\)
3 \(\mathrm{\dfrac{q}{w}}\)
4 \(\mathrm{q+w}\)
Explanation:
\(\mathrm{q+w=\Delta U}\) is a state function.
CHXI06:THERMODYNAMICS
369148
Which of the following are not state functions? (I) \(\mathrm{q+w}\) (II) \(\mathrm{q}\) (III) w (IV) H-TS
1 (I) and (IV)
2 (II), (III) and (IV)
3 (I), (II) and (III)
4 (II) and (III)
Explanation:
We know that heat (q) and work (w) are not state functions but \(\mathrm{(\mathrm{q}+\mathrm{w})}\) is a state function. \({\rm{H - TS}}\) (i.e. G) is also a state function.
CHXI06:THERMODYNAMICS
369149
Statement A : T, P and V are state variables or state functions. Statement B : Their values depend on the state of the system and not on how it is reached.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Values of state functions depend only on the state of the system and not on how it is reached.
CHXI06:THERMODYNAMICS
369150
In a change from state \(\mathrm{A}\) to state \(\mathrm{B}\) :
1 " \({\text{q}}\)" depends only on the initial and final states.
2 "\({\text{W}}\)" depends only on the initial and final states.
3 \(\Delta \mathrm{E}\) depends only on the initial and final states.
4 \(\Delta\)\({\text{E}}\) depends upon the path adopted by " \({\text{A}}\) " to change into " \({\text{B}}\) "
Explanation:
Because \(\Delta \mathrm{E}\) is a state function. Heat and work are path functions.
369146
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. The conditions are
1 High Temperature, High Pressure
2 Constant Temperature, Constant Pressure
3 Low Temperature, Low Pressure
4 Constant Volume, Constant Pressure
Explanation:
By first law of thermodynamics: \(\mathrm{q=\Delta U+(-w)}\) \(\mathrm{(-w)=p \Delta V}\) \(\mathrm{\therefore q=\Delta U+p \Delta V}\) \(\mathrm{\Delta V=0}\), since volume is constant. \(\mathrm{\therefore q_{v}=\Delta U+0}\) \(\mathrm{\Rightarrow q_{v}=\Delta U=}\) change in internal energy At constant pressure \(\mathrm{q_{p}=\Delta U+p \Delta V}\) But, \(\mathrm{\Delta U+p \Delta V=\Delta H}\) \(\mathrm{\therefore q_{p}=\Delta H=}\) change in enthalpy So, at constant volume and at constant pressure heat change is a state function because it is equal to change in internal energy and change in enthalpy respectively which are state functions.
CHXI06:THERMODYNAMICS
369147
Identify the state function among the following:
1 \(\mathrm{q}\)
2 \(\mathrm{q-w}\)
3 \(\mathrm{\dfrac{q}{w}}\)
4 \(\mathrm{q+w}\)
Explanation:
\(\mathrm{q+w=\Delta U}\) is a state function.
CHXI06:THERMODYNAMICS
369148
Which of the following are not state functions? (I) \(\mathrm{q+w}\) (II) \(\mathrm{q}\) (III) w (IV) H-TS
1 (I) and (IV)
2 (II), (III) and (IV)
3 (I), (II) and (III)
4 (II) and (III)
Explanation:
We know that heat (q) and work (w) are not state functions but \(\mathrm{(\mathrm{q}+\mathrm{w})}\) is a state function. \({\rm{H - TS}}\) (i.e. G) is also a state function.
CHXI06:THERMODYNAMICS
369149
Statement A : T, P and V are state variables or state functions. Statement B : Their values depend on the state of the system and not on how it is reached.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
Values of state functions depend only on the state of the system and not on how it is reached.
CHXI06:THERMODYNAMICS
369150
In a change from state \(\mathrm{A}\) to state \(\mathrm{B}\) :
1 " \({\text{q}}\)" depends only on the initial and final states.
2 "\({\text{W}}\)" depends only on the initial and final states.
3 \(\Delta \mathrm{E}\) depends only on the initial and final states.
4 \(\Delta\)\({\text{E}}\) depends upon the path adopted by " \({\text{A}}\) " to change into " \({\text{B}}\) "
Explanation:
Because \(\Delta \mathrm{E}\) is a state function. Heat and work are path functions.
