Measuring thermal quantities by the method of mixtures - class-XI
| Description: measuring thermal quantities by the method of mixtures | |
| Number of Questions: 74 | |
| Created by: Anumati Koshy | |
| Tags: physics thermal physics heat calorimetry heat and thermodynamics heat and temperature thermal properties thermal properties of matter properties of bulk matter measurement and effects of heat |
How much heat is required to raise the temperature of 150 g of iron from $20 ^oC$ to $25 ^oC$? (Specific heat of iron $480 J kg^{-1} {\;}^oC^{-1})$
Find the heat lost by a copper cube of mass 400 g when it cool from $100^oC$ to $30^oC$. (Specific of heat of copper $=390 J kg^{-1} {\;}^oC^{-1})$.
A body having 1680 J of energy is supplied to 1000 g of water. If the entire amount of energy is converted into heat, the rise in temperature of water (sp. heat of water $=4200 J kg^{-1} {\;}^oC^{-1})$
What is the process in which heat energy of both hot and cold body equalizes?
How much heat is required to raise the temperature of 100 g of water of $5 ^oC$ to $95 ^oC$?
According to principle of calorimetry, heat absorbed by cold bodies is equal to heat released by hot bodies.
5 kg of water at $80^oC$ is taken in a bucket of negligible heat capacity, 15 kg of water at $20^oC$ is added to it. What is the temperature of the mixture?
5 g of water at $30^oC$ and 5 g of ice at $-20^oC$ are mixed together in a calorimeter. What is the final temperature of the mixture. Given specific heat of ice $=0.5 cal g^{-1} (^oC)^{-1}$ and latent heat of fusion of ice $=80 cal g^{-1}$.
In a process 10 g of ice at $-5^oC$ is converted into the steam at $100^oC$. If specific heat of ice is $0.5 \ cal g^{-1} {\;}^oC^{-1}$, then the amount of heat required to convert 10 g of ice from $-5^oC$ to $0^oC$ is :
400 g of ice at 253 K is mixed with 0.05 kg of steam at $100^oC$. Latent heat of vaporisation of steam $=540 cal g^{-1}$. Latent heat of fusion of ice $=80 cal g^{-1}$. Specific heat of ice $=0.5 cal g^{-1} {\;}^oC^{-1}$. Find the resultant temperature of the mixture.
A piece of copper weighing 500 g is heated to $100^oC$ and dropped into 200g of water at $25^oC$. Find the temperature of the mixture. The specific heat of Cu is $0.42 J g^{-1} {\;}^oC^{-1}$.
$10\ kg$ of hot water in a bucket at $70^oC$ is cooled for taking a bath adding to it $20\ kg$ water at $20^oC$. What is the temperature of the mixture? (Neglect the thermal capacity of the bucket)
What is the final temperature of the mixture of 300 g of water at $25^oC$ added to 100 of ice at $0^oC$.
500 g of water at $100^oC$ is mixed with 300 g at $30^oC$. Find the temperature of the mixture. Specific heat of water $=4.2 J g^{-1} {\;}^oC^{-1}$.
A calorimeter contains $70.2 \,g$ of water at $15.3^o C$. If $143.7 \,g$ of water at $36.5^o C$ in mixed it with the common temperature is $28.7^o C$. The water equivalent of the calorimeter is:
$5$g of copper was heated from $20^{\circ}$ to $80^{\circ}$. How much energy was used to heat Cu? (Specific heat capacity of Cu is $0.092 cal/g ^{\circ}C$).
A calorimeter constains 10 g of water at ${ 20 }^{ \circ }$ C. The temperature falls to ${ 15 }^{ \circ }$ C in 10 min. When calorimeter contains 20 g of water at ${ 20 }^{ \circ }$ C, it takes 15 min for the temperature to become ${ 15 }^{ \circ }$ C. The water equivalent of the calorimeter is
What is the principle of the method of a mixture? Name the law on which this principle is based.
In a calorimeter of water equivalent $20 { g },$ water of mass $1.1 { kg }$ is taken at $288{ K }$ temperature. If steam at temperature $373 { K }$ is passed through it and temperature of water increases by $6.5 ^ { \circ } { C }$ then the mass of steam condensed is
2000 J of energy is needed to heat 1 kg of paraffin through $1^{\circ}C$. So How much energy is needed to heat 10 kg of paraffin through $2^{\circ}C$ ?
When in thermal contact, the quantity of heat lost by the hotter body is ...... the amount of heat gained by the colder body. (neglect loss of heat due to convection & radiation)
Bunty mixed 440 gm of ice at $0^{\circ}C$ with 540 gm of water at $80^{\circ} C$ in a bowl. Then what would remain after sometime in the bowl?
The quantity of heat required to raise the temperature of 2000 g of water from 10$^o$C to 50$^o$C is
The quantity/ quantities that does/do not have mass in its/their dimensions is/are
When 60 calories of heat are supplied to 15 g of water, the rise in temperature is
Calorimeters are generally made of
On which law does the study of calorimetry based?
When 60 calories of heat are supplied to 15 g of water, the rise in temperature is
A thermos bottle containing coffee is vigorously shaken. If the coffee is considered as a system, then the temperature of the coffee will
The branch of physics that deals with the measurement of heat energy is known as
A thermometer is used to measure
Which of the following properties must be known in order to calculate the amount of heat needed to melt 1.0kg of ice at $0^oC$?
I. The specific heat of water
II. The latent heat of fusion for water
III. The density of water.
Heat is added to a block of ice of mass $m$ until the entire block melts into liquid water. Identify by which of the following method this can be explained ?
State True or False.
400 g of vegetable oil of specific heat capacity 1.98 J ${ g }^{ -1 }$ $^{ \circ }{ { C }^{ -1 } }$) is cooled from ${ 100 }^{ \circ }C$. Find the final temperature, if the heat energy given out by is 47376 J.
How much heat is required to raise the temperature of $150 g$ of iron from ${ 20 }^{ \circ }C$ to ${ 25 }^{ \circ }C$?
How much heat is required to raise the temperature of $100 g$ of water from ${ 5 }^{ \circ }C$ to ${ 95 }^{ \circ }C$?
2000 cal of heat is supplied to 200 g of water. Find the rise in temperature. (Specific heat of water = 1 cal ${ { g }^{ -1 } }^{ \circ }{ C }^{ -1 }$)
What will be the amount of heat required to convert $50 g$ of ice at ${ 0 }^{ \circ }C$ to water at ${ 0 }^{ \circ }C$?
Calculate the quantity of heat required to convert 1.5 kg of ice at ${ 100 }^{ \circ }C$ to water at ${ 15 }^{ \circ }C$. (${ L } _{ ice }\quad =\quad 3.34\quad \times \quad { 10 }^{ 5 }\quad J{ \quad kg }^{ -1 }$, ${ C } _{ water }\quad =\quad 4180\quad J{ \quad kg }^{ -1 }\quad ^{ \circ }{ { C }^{ -1 } }$)
One calorie is defined as the heat required to raise the temperature of $1$ gm of water by $1^o$C in a certain interval of temperature and at certain pressure. The temperature interval and pressure is?
If there are no heat losses to the surroundings, the quantity of heat gained by the cold body is equal to the quantity of heat lost by the hot body.
A copper ball of mass $100gm$ is at a temperature $T$. It is dropped in a copper calorimeter of mass $100gm$, filled with $170gm$ of water at room temperature. Subsequently the temperature of the system is found to b4 ${75}^{o}$. $T$ is given by then (Given: room temperature $={30}^{o}C$, specific heat of copper $=0.1cal/gm _{ }^{ o }{ C }\quad $)
400 g of vegetable oil of specific heat capacity $1.98 J g^{-1} {\;}^oC^{-1}$ is cooled from $100^oC$. Find the final temperature, if the heat energy given out by oil is 47376 J.
2000 cal of heat is supplied to 200 g of water. Find the rise in temperature. (Specific heat of water $=1 cal g^{-1} {\;}^oC^{-1})$
500 g of hot water at $60^oC$ is kept in the open till its temperature falls to $40^oC$. Calculate the heat energy lost to the surroundings by the water. (Specific heat of water $=4200 J kg^{-1} {\;}^oC^{-1})$
How much amount of heat is required to raise the temperature of 100 g of water from $30 ^oC$ to $100 ^oC$? The specific heat of water $=4.2 J g^{-1} {\;}^oC^{-1}$.
What quantity of heat would be given out by 200 gm of copper in cooling from $80^oC$ to $20^oC$ (Specific heat of copper $=0.09 cal g^{-1} {\;}^oC^{-1})$?
If $20 \ g$ of ice at $0^\circ C$ is mixed with $10 \ g$ of water at $40^\circ C$, the final mass of water in the mixture is:
A liquid P if specific heat capacity $2400 J kg^{-1} K^{-1}$ and at $70^oC$ is mixed with another liquid R of specific heat capacity $1000 J kg^{-1} K^{-1}$ at $30^oC$. After mixing, the final temperature of the mixture is $40^oC$. Find the ratio of the mass of the liquids mixed?
Calculate the amount of heat required to convert 5 kg of ice to $0^oC$ to vapour at $100^oC$.
In a calorimeter of water equivalent $20g$,water of mass $1.1$kg is taken at $288K$ temperature.If steam at temperature $373K$ is passed through it and temperature of water increases by $6.5^oC$ then the mass of steam condensed is:
Steam at $100^oC$ is passed into $2.0$kg of water contained in a calorimeter of water equivalent $0.02$kg at $15^oC$ till the temperature of the calorimeter and its content rise to $90^oC$. The mass of steam condensed in kg is
Utensils used for efficient cooking should have
A copper calorimeter of a mass $300\ g$ contains $500\ g$ of water at a temperature of $20^\circ C$. A $500\ g$ of copper block at $100^\circ C$ is dropped into the calorimeter. If the resultant temperature is $25^\circ C$, then fond the specific heat of copper in $JKg^{-1} K^{-1}$.
Calories is defined as the amount of heat required to rise temperature of $1\ g$ of water by $1^{o}C$ and it is defined under which of the following conditions.
A copper calorimeter contains $100 g$ of water at $16^o C$. When $15 g$ of ice is added to it, the resultant temperature of the mixture is $4^o C$. Water equivalent of the calorimeter is
Which of the following material is used to make calorimeter?
The water equivalent of a 400 g copper calorimeter (specific heat =0.1 cal/$g^{ o }C$)-
A man would feel iron and wooden balls equally cold or hot at
How many calories of heat are required by gram of water at $99^oC$ to boil off:
$50 g$ of ice at 0 C is mixed with $50 g$ of water at 20 C.The resultant temperature of the mixture would be
At which temperature do the readings of the celcius and the Fahrenheit scales coincide ?
The amount of heat required to convert 1 g of ice (specific 0.5 cal at $g^{-1o} C^{-1}$ ) at $-10^0 C$ to steam at $100 $ $^\circ C$ is ___________.
The specific heat for substance $A$ is twice the specific heat of substance $B$. The same mass of each substance is allowed to gain $50$ Joules of heat energy. As a result of the heating process:
To measure the specific heat of copper, an experiment is performed in the lab. A piece of copper is heated in an oven then dropped into a beaker of water. To calculate the specific heat of copper, the experimenter must know or measure the value of all of the quantities below EXCEPT the
An aluminium block of 2m mass and an iron block of m mass,each absorbs the same amount of heat, and both blocks remain solid. If the specific heat of aluminium is twice the specific heat of iron, then find out the correct statement?
A mass of stainless steel spoon is 0.04 kg and specific heat is $0.50 kJ/kg \times ^oC$. Then calculate the heat which is required to raise the temperature $20^oC$ to $50^oC$ of the spoon.
A body having $1680 J$ of energy is supplied to $100 g$ of water. If the entire amount of energy is converted into heat the rise in temperature of water (sp. heat of water = $4200 JKg^{ -1 }\ ^0C ^{ -1 } $)
$5gm$ of steam at $100^oC$ is passed into calorimeter containing liquid , Temperature of liquid rises from $32^oC$ to $40^oC$. Then water equivalent of calorimeter and content is
1 kg of water at $20^{\circ}C$ is, mixed with 800 g of water at $80^{\circ}C$. Assuming that no heat is lost to the surroundings. Calculate the final temperature of the mixture.
The temperature of equal masses of three different liquids A, B, and C are $12^o C$,$19^o C$ and $28^o C$ respectively. The temperature when A and B are mixed is $16^oC$ and When B and C are mixed is $23^o C$. The temperature when A and C are mixed is:
An adulterated sample of milk has a density, 1032 kg m$^{-3}$, while pure milk has a density of 1080 kg m$^{-3}$. Then the volume of pure milk in a sampled of 10 litres of adulterated milk is:
An experiment requires a gas with $\gamma = 1.50$. This can be achieved by mixing together monatomic and rigid diatomic ideal gases. The ratio of moles of the monatomic to diatomic gas in the mixture is