369330
A system is provided \(\mathrm{50 \mathrm{~J}}\) of heat and work done on the system is \(\mathrm{10 \mathrm{~J}}\). The change in internal energy during the process is
369331
During a process, system absorbs \(710 \mathrm{~J}\) of heat and increases the internal energy by \(460 \mathrm{~J}\). What is the work performed by system?
1 \(-250 \mathrm{~J}\)
2 \(-1170 \mathrm{~J}\)
3 \(-710 \mathrm{~J}\)
4 \(-460 \mathrm{~J}\)
Explanation:
\(\mathrm{Q}=710 \mathrm{~J}\) (heat given to system), \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) According to first law of thermodynamics \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& \therefore \mathrm{W}=\Delta \mathrm{U}-\mathrm{Q} \\& =460-710=-250 \mathrm{~J}\end{aligned}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369332
"The mass and energy both are conserved in an isolated system", is the statement of
1 second law of thermodynamics
2 third law of thermodynamcis
3 modified first law of thermodynamics
4 first law of thermodynamics
Explanation:
"The mass and energy both are conserved in an isolated system", is the statement of modified first law of thermodynamics. According to this law, if a certain amount of one kind of energy is produced, an equal amount of some other kind of energy is consumed so that the total energy in the universe remains constant.
MHTCET - 2019
CHXI06:THERMODYNAMICS
369333
What is internal energy change when \(62 \mathrm{~J}\) of work is done on the sytem and \(128 \mathrm{~J}\) of heat is transferred to surrounding?
1 \(-62 \mathrm{~J}\)
2 \(-190 \mathrm{~J}\)
3 \(-128 \mathrm{~J}\)
4 \(-66 J\)
Explanation:
Workdone on the system, so \({\text{ + ve}}\) \(\mathrm{W}=62 \mathrm{~J}\). Heat is given out, so \({\text{ - ve}}\) \(\mathrm{Q}=-128 \mathrm{~J}\) According to first law of thermodynamics, \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& =-128+62=-66 \mathrm{~J}\end{aligned}\)
369330
A system is provided \(\mathrm{50 \mathrm{~J}}\) of heat and work done on the system is \(\mathrm{10 \mathrm{~J}}\). The change in internal energy during the process is
369331
During a process, system absorbs \(710 \mathrm{~J}\) of heat and increases the internal energy by \(460 \mathrm{~J}\). What is the work performed by system?
1 \(-250 \mathrm{~J}\)
2 \(-1170 \mathrm{~J}\)
3 \(-710 \mathrm{~J}\)
4 \(-460 \mathrm{~J}\)
Explanation:
\(\mathrm{Q}=710 \mathrm{~J}\) (heat given to system), \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) According to first law of thermodynamics \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& \therefore \mathrm{W}=\Delta \mathrm{U}-\mathrm{Q} \\& =460-710=-250 \mathrm{~J}\end{aligned}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369332
"The mass and energy both are conserved in an isolated system", is the statement of
1 second law of thermodynamics
2 third law of thermodynamcis
3 modified first law of thermodynamics
4 first law of thermodynamics
Explanation:
"The mass and energy both are conserved in an isolated system", is the statement of modified first law of thermodynamics. According to this law, if a certain amount of one kind of energy is produced, an equal amount of some other kind of energy is consumed so that the total energy in the universe remains constant.
MHTCET - 2019
CHXI06:THERMODYNAMICS
369333
What is internal energy change when \(62 \mathrm{~J}\) of work is done on the sytem and \(128 \mathrm{~J}\) of heat is transferred to surrounding?
1 \(-62 \mathrm{~J}\)
2 \(-190 \mathrm{~J}\)
3 \(-128 \mathrm{~J}\)
4 \(-66 J\)
Explanation:
Workdone on the system, so \({\text{ + ve}}\) \(\mathrm{W}=62 \mathrm{~J}\). Heat is given out, so \({\text{ - ve}}\) \(\mathrm{Q}=-128 \mathrm{~J}\) According to first law of thermodynamics, \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& =-128+62=-66 \mathrm{~J}\end{aligned}\)
369330
A system is provided \(\mathrm{50 \mathrm{~J}}\) of heat and work done on the system is \(\mathrm{10 \mathrm{~J}}\). The change in internal energy during the process is
369331
During a process, system absorbs \(710 \mathrm{~J}\) of heat and increases the internal energy by \(460 \mathrm{~J}\). What is the work performed by system?
1 \(-250 \mathrm{~J}\)
2 \(-1170 \mathrm{~J}\)
3 \(-710 \mathrm{~J}\)
4 \(-460 \mathrm{~J}\)
Explanation:
\(\mathrm{Q}=710 \mathrm{~J}\) (heat given to system), \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) According to first law of thermodynamics \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& \therefore \mathrm{W}=\Delta \mathrm{U}-\mathrm{Q} \\& =460-710=-250 \mathrm{~J}\end{aligned}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369332
"The mass and energy both are conserved in an isolated system", is the statement of
1 second law of thermodynamics
2 third law of thermodynamcis
3 modified first law of thermodynamics
4 first law of thermodynamics
Explanation:
"The mass and energy both are conserved in an isolated system", is the statement of modified first law of thermodynamics. According to this law, if a certain amount of one kind of energy is produced, an equal amount of some other kind of energy is consumed so that the total energy in the universe remains constant.
MHTCET - 2019
CHXI06:THERMODYNAMICS
369333
What is internal energy change when \(62 \mathrm{~J}\) of work is done on the sytem and \(128 \mathrm{~J}\) of heat is transferred to surrounding?
1 \(-62 \mathrm{~J}\)
2 \(-190 \mathrm{~J}\)
3 \(-128 \mathrm{~J}\)
4 \(-66 J\)
Explanation:
Workdone on the system, so \({\text{ + ve}}\) \(\mathrm{W}=62 \mathrm{~J}\). Heat is given out, so \({\text{ - ve}}\) \(\mathrm{Q}=-128 \mathrm{~J}\) According to first law of thermodynamics, \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& =-128+62=-66 \mathrm{~J}\end{aligned}\)
369330
A system is provided \(\mathrm{50 \mathrm{~J}}\) of heat and work done on the system is \(\mathrm{10 \mathrm{~J}}\). The change in internal energy during the process is
369331
During a process, system absorbs \(710 \mathrm{~J}\) of heat and increases the internal energy by \(460 \mathrm{~J}\). What is the work performed by system?
1 \(-250 \mathrm{~J}\)
2 \(-1170 \mathrm{~J}\)
3 \(-710 \mathrm{~J}\)
4 \(-460 \mathrm{~J}\)
Explanation:
\(\mathrm{Q}=710 \mathrm{~J}\) (heat given to system), \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) \(\Delta \mathrm{U}=460 \mathrm{~J}(\) increase in internal energy \()\) According to first law of thermodynamics \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& \therefore \mathrm{W}=\Delta \mathrm{U}-\mathrm{Q} \\& =460-710=-250 \mathrm{~J}\end{aligned}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS
369332
"The mass and energy both are conserved in an isolated system", is the statement of
1 second law of thermodynamics
2 third law of thermodynamcis
3 modified first law of thermodynamics
4 first law of thermodynamics
Explanation:
"The mass and energy both are conserved in an isolated system", is the statement of modified first law of thermodynamics. According to this law, if a certain amount of one kind of energy is produced, an equal amount of some other kind of energy is consumed so that the total energy in the universe remains constant.
MHTCET - 2019
CHXI06:THERMODYNAMICS
369333
What is internal energy change when \(62 \mathrm{~J}\) of work is done on the sytem and \(128 \mathrm{~J}\) of heat is transferred to surrounding?
1 \(-62 \mathrm{~J}\)
2 \(-190 \mathrm{~J}\)
3 \(-128 \mathrm{~J}\)
4 \(-66 J\)
Explanation:
Workdone on the system, so \({\text{ + ve}}\) \(\mathrm{W}=62 \mathrm{~J}\). Heat is given out, so \({\text{ - ve}}\) \(\mathrm{Q}=-128 \mathrm{~J}\) According to first law of thermodynamics, \(\begin{aligned}& \Delta \mathrm{U}=\mathrm{Q}+\mathrm{W} \\& =-128+62=-66 \mathrm{~J}\end{aligned}\)
