148196
$1 \mathrm{~g}$ of ice is mixed with $1 \mathrm{~g}$ of steam. At thermal equilibrium, the temperature of the mixture is :
1 $50^{\circ} \mathrm{C}$
2 $0^{\circ} \mathrm{C}$
3 $55^{\circ} \mathrm{C}$
4 $100^{\circ} \mathrm{C}$
Explanation:
D According to principle of calorimeter state that total heat given by a hotter body is equal to the total heat received by colder body. i.e. Heat required to melt $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $0^{\circ} \mathrm{C}$ is $80 \mathrm{cal}$. And Heat required to convert $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $100^{\circ} \mathrm{C}=1 \times 1 \times 100=100 \mathrm{cal}$ Heat required to condense $1 \mathrm{~g}$ of steam $=1 \times 540 \mathrm{cal}=$ 540 cal clearly, whole of steam is not condensed so, temperature of the mixture is $100^{\circ} \mathrm{C}$.
Karnataka CET-2015
Thermodynamics
148220
An ice-cream has a marked value of 350 cal. Energy delivered by this ice-cream to the body is (The calorie in this case is a kilocaloric)
1 $0.407 \mathrm{kWh}$
2 $3.50 \mathrm{kWh}$
3 $1.750 \mathrm{kWh}$
4 $7.00 \mathrm{kWh}$
Explanation:
A Amount of energy delivered by given ice cream to the body $=350 \mathrm{cal}$. To find kilowatt-hour of energy deliver to the body We know that, $1 \mathrm{kcal}=10^{3}$ calorie $=4200 \mathrm{~J}=\frac{4200}{3.6 \times 10^{6}} \mathrm{kWh}$ Now according to the question, $350 \mathrm{kcal} =\frac{350 \times 4200}{3.6 \times 10^{6}} \mathrm{kWh}$ $=0.407 \mathrm{kWh}$
AMU-2003
Thermodynamics
148203
During the melting of a slab of ice at $273 \mathrm{~K}$ at atmospheric pressure
1 Positive work is done by the ice water system on the atmosphere
2 positive work is done on the ice water system by the atmosphere
3 internal energy of ice water system decreases
4 None of the above
Explanation:
B There is a decrease in volume during melting of an ice slab at $273 \mathrm{~K}$. Therefore, negative work is done on the by ice water system atmosphere or positive work is done on the ice-water system by the atmosphere.
UP CPMT-2006
Thermodynamics
148179
The degrees of freedom of a molecule of a triatomic gas are:
1 2
2 4
3 6
4 8
Explanation:
C Degree of freedom for triatomic gas is 6 .
BCECE-2005
Thermodynamics
148183
Two blocks of ice when pressed together join to form one block because
1 of heat produced during pressing
2 of cold produced during pressing
3 melting point of ice decreases with increase of pressure
4 melting point of ice increases with increase in pressure
Explanation:
C Two blocks of ice when pressed together join to form one block because melting point of ice decreases with increase of pressure.
148196
$1 \mathrm{~g}$ of ice is mixed with $1 \mathrm{~g}$ of steam. At thermal equilibrium, the temperature of the mixture is :
1 $50^{\circ} \mathrm{C}$
2 $0^{\circ} \mathrm{C}$
3 $55^{\circ} \mathrm{C}$
4 $100^{\circ} \mathrm{C}$
Explanation:
D According to principle of calorimeter state that total heat given by a hotter body is equal to the total heat received by colder body. i.e. Heat required to melt $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $0^{\circ} \mathrm{C}$ is $80 \mathrm{cal}$. And Heat required to convert $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $100^{\circ} \mathrm{C}=1 \times 1 \times 100=100 \mathrm{cal}$ Heat required to condense $1 \mathrm{~g}$ of steam $=1 \times 540 \mathrm{cal}=$ 540 cal clearly, whole of steam is not condensed so, temperature of the mixture is $100^{\circ} \mathrm{C}$.
Karnataka CET-2015
Thermodynamics
148220
An ice-cream has a marked value of 350 cal. Energy delivered by this ice-cream to the body is (The calorie in this case is a kilocaloric)
1 $0.407 \mathrm{kWh}$
2 $3.50 \mathrm{kWh}$
3 $1.750 \mathrm{kWh}$
4 $7.00 \mathrm{kWh}$
Explanation:
A Amount of energy delivered by given ice cream to the body $=350 \mathrm{cal}$. To find kilowatt-hour of energy deliver to the body We know that, $1 \mathrm{kcal}=10^{3}$ calorie $=4200 \mathrm{~J}=\frac{4200}{3.6 \times 10^{6}} \mathrm{kWh}$ Now according to the question, $350 \mathrm{kcal} =\frac{350 \times 4200}{3.6 \times 10^{6}} \mathrm{kWh}$ $=0.407 \mathrm{kWh}$
AMU-2003
Thermodynamics
148203
During the melting of a slab of ice at $273 \mathrm{~K}$ at atmospheric pressure
1 Positive work is done by the ice water system on the atmosphere
2 positive work is done on the ice water system by the atmosphere
3 internal energy of ice water system decreases
4 None of the above
Explanation:
B There is a decrease in volume during melting of an ice slab at $273 \mathrm{~K}$. Therefore, negative work is done on the by ice water system atmosphere or positive work is done on the ice-water system by the atmosphere.
UP CPMT-2006
Thermodynamics
148179
The degrees of freedom of a molecule of a triatomic gas are:
1 2
2 4
3 6
4 8
Explanation:
C Degree of freedom for triatomic gas is 6 .
BCECE-2005
Thermodynamics
148183
Two blocks of ice when pressed together join to form one block because
1 of heat produced during pressing
2 of cold produced during pressing
3 melting point of ice decreases with increase of pressure
4 melting point of ice increases with increase in pressure
Explanation:
C Two blocks of ice when pressed together join to form one block because melting point of ice decreases with increase of pressure.
148196
$1 \mathrm{~g}$ of ice is mixed with $1 \mathrm{~g}$ of steam. At thermal equilibrium, the temperature of the mixture is :
1 $50^{\circ} \mathrm{C}$
2 $0^{\circ} \mathrm{C}$
3 $55^{\circ} \mathrm{C}$
4 $100^{\circ} \mathrm{C}$
Explanation:
D According to principle of calorimeter state that total heat given by a hotter body is equal to the total heat received by colder body. i.e. Heat required to melt $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $0^{\circ} \mathrm{C}$ is $80 \mathrm{cal}$. And Heat required to convert $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $100^{\circ} \mathrm{C}=1 \times 1 \times 100=100 \mathrm{cal}$ Heat required to condense $1 \mathrm{~g}$ of steam $=1 \times 540 \mathrm{cal}=$ 540 cal clearly, whole of steam is not condensed so, temperature of the mixture is $100^{\circ} \mathrm{C}$.
Karnataka CET-2015
Thermodynamics
148220
An ice-cream has a marked value of 350 cal. Energy delivered by this ice-cream to the body is (The calorie in this case is a kilocaloric)
1 $0.407 \mathrm{kWh}$
2 $3.50 \mathrm{kWh}$
3 $1.750 \mathrm{kWh}$
4 $7.00 \mathrm{kWh}$
Explanation:
A Amount of energy delivered by given ice cream to the body $=350 \mathrm{cal}$. To find kilowatt-hour of energy deliver to the body We know that, $1 \mathrm{kcal}=10^{3}$ calorie $=4200 \mathrm{~J}=\frac{4200}{3.6 \times 10^{6}} \mathrm{kWh}$ Now according to the question, $350 \mathrm{kcal} =\frac{350 \times 4200}{3.6 \times 10^{6}} \mathrm{kWh}$ $=0.407 \mathrm{kWh}$
AMU-2003
Thermodynamics
148203
During the melting of a slab of ice at $273 \mathrm{~K}$ at atmospheric pressure
1 Positive work is done by the ice water system on the atmosphere
2 positive work is done on the ice water system by the atmosphere
3 internal energy of ice water system decreases
4 None of the above
Explanation:
B There is a decrease in volume during melting of an ice slab at $273 \mathrm{~K}$. Therefore, negative work is done on the by ice water system atmosphere or positive work is done on the ice-water system by the atmosphere.
UP CPMT-2006
Thermodynamics
148179
The degrees of freedom of a molecule of a triatomic gas are:
1 2
2 4
3 6
4 8
Explanation:
C Degree of freedom for triatomic gas is 6 .
BCECE-2005
Thermodynamics
148183
Two blocks of ice when pressed together join to form one block because
1 of heat produced during pressing
2 of cold produced during pressing
3 melting point of ice decreases with increase of pressure
4 melting point of ice increases with increase in pressure
Explanation:
C Two blocks of ice when pressed together join to form one block because melting point of ice decreases with increase of pressure.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
Thermodynamics
148196
$1 \mathrm{~g}$ of ice is mixed with $1 \mathrm{~g}$ of steam. At thermal equilibrium, the temperature of the mixture is :
1 $50^{\circ} \mathrm{C}$
2 $0^{\circ} \mathrm{C}$
3 $55^{\circ} \mathrm{C}$
4 $100^{\circ} \mathrm{C}$
Explanation:
D According to principle of calorimeter state that total heat given by a hotter body is equal to the total heat received by colder body. i.e. Heat required to melt $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $0^{\circ} \mathrm{C}$ is $80 \mathrm{cal}$. And Heat required to convert $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $100^{\circ} \mathrm{C}=1 \times 1 \times 100=100 \mathrm{cal}$ Heat required to condense $1 \mathrm{~g}$ of steam $=1 \times 540 \mathrm{cal}=$ 540 cal clearly, whole of steam is not condensed so, temperature of the mixture is $100^{\circ} \mathrm{C}$.
Karnataka CET-2015
Thermodynamics
148220
An ice-cream has a marked value of 350 cal. Energy delivered by this ice-cream to the body is (The calorie in this case is a kilocaloric)
1 $0.407 \mathrm{kWh}$
2 $3.50 \mathrm{kWh}$
3 $1.750 \mathrm{kWh}$
4 $7.00 \mathrm{kWh}$
Explanation:
A Amount of energy delivered by given ice cream to the body $=350 \mathrm{cal}$. To find kilowatt-hour of energy deliver to the body We know that, $1 \mathrm{kcal}=10^{3}$ calorie $=4200 \mathrm{~J}=\frac{4200}{3.6 \times 10^{6}} \mathrm{kWh}$ Now according to the question, $350 \mathrm{kcal} =\frac{350 \times 4200}{3.6 \times 10^{6}} \mathrm{kWh}$ $=0.407 \mathrm{kWh}$
AMU-2003
Thermodynamics
148203
During the melting of a slab of ice at $273 \mathrm{~K}$ at atmospheric pressure
1 Positive work is done by the ice water system on the atmosphere
2 positive work is done on the ice water system by the atmosphere
3 internal energy of ice water system decreases
4 None of the above
Explanation:
B There is a decrease in volume during melting of an ice slab at $273 \mathrm{~K}$. Therefore, negative work is done on the by ice water system atmosphere or positive work is done on the ice-water system by the atmosphere.
UP CPMT-2006
Thermodynamics
148179
The degrees of freedom of a molecule of a triatomic gas are:
1 2
2 4
3 6
4 8
Explanation:
C Degree of freedom for triatomic gas is 6 .
BCECE-2005
Thermodynamics
148183
Two blocks of ice when pressed together join to form one block because
1 of heat produced during pressing
2 of cold produced during pressing
3 melting point of ice decreases with increase of pressure
4 melting point of ice increases with increase in pressure
Explanation:
C Two blocks of ice when pressed together join to form one block because melting point of ice decreases with increase of pressure.
148196
$1 \mathrm{~g}$ of ice is mixed with $1 \mathrm{~g}$ of steam. At thermal equilibrium, the temperature of the mixture is :
1 $50^{\circ} \mathrm{C}$
2 $0^{\circ} \mathrm{C}$
3 $55^{\circ} \mathrm{C}$
4 $100^{\circ} \mathrm{C}$
Explanation:
D According to principle of calorimeter state that total heat given by a hotter body is equal to the total heat received by colder body. i.e. Heat required to melt $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $0^{\circ} \mathrm{C}$ is $80 \mathrm{cal}$. And Heat required to convert $1 \mathrm{~g}$ of ice $0^{\circ} \mathrm{C}$ into $1 \mathrm{~g}$ of water at $100^{\circ} \mathrm{C}=1 \times 1 \times 100=100 \mathrm{cal}$ Heat required to condense $1 \mathrm{~g}$ of steam $=1 \times 540 \mathrm{cal}=$ 540 cal clearly, whole of steam is not condensed so, temperature of the mixture is $100^{\circ} \mathrm{C}$.
Karnataka CET-2015
Thermodynamics
148220
An ice-cream has a marked value of 350 cal. Energy delivered by this ice-cream to the body is (The calorie in this case is a kilocaloric)
1 $0.407 \mathrm{kWh}$
2 $3.50 \mathrm{kWh}$
3 $1.750 \mathrm{kWh}$
4 $7.00 \mathrm{kWh}$
Explanation:
A Amount of energy delivered by given ice cream to the body $=350 \mathrm{cal}$. To find kilowatt-hour of energy deliver to the body We know that, $1 \mathrm{kcal}=10^{3}$ calorie $=4200 \mathrm{~J}=\frac{4200}{3.6 \times 10^{6}} \mathrm{kWh}$ Now according to the question, $350 \mathrm{kcal} =\frac{350 \times 4200}{3.6 \times 10^{6}} \mathrm{kWh}$ $=0.407 \mathrm{kWh}$
AMU-2003
Thermodynamics
148203
During the melting of a slab of ice at $273 \mathrm{~K}$ at atmospheric pressure
1 Positive work is done by the ice water system on the atmosphere
2 positive work is done on the ice water system by the atmosphere
3 internal energy of ice water system decreases
4 None of the above
Explanation:
B There is a decrease in volume during melting of an ice slab at $273 \mathrm{~K}$. Therefore, negative work is done on the by ice water system atmosphere or positive work is done on the ice-water system by the atmosphere.
UP CPMT-2006
Thermodynamics
148179
The degrees of freedom of a molecule of a triatomic gas are:
1 2
2 4
3 6
4 8
Explanation:
C Degree of freedom for triatomic gas is 6 .
BCECE-2005
Thermodynamics
148183
Two blocks of ice when pressed together join to form one block because
1 of heat produced during pressing
2 of cold produced during pressing
3 melting point of ice decreases with increase of pressure
4 melting point of ice increases with increase in pressure
Explanation:
C Two blocks of ice when pressed together join to form one block because melting point of ice decreases with increase of pressure.