Hot water kept in a beaker placed in a room cools from $ 70{}^\circ C $ to $ 60{}^\circ C $ in 4 minutes. The time taken by it to cool from $ 69{}^\circ C $ to $ ~59{}^\circ C $ will be:
- the same 4 minutes
- more than 4 minutes
- less than 4 minutes
- we cannot say definitely
The Correct Option is B
Solution and Explanation
Top Questions on Calorimetry
- 40 g of water at 40°C is added to 10 g of water at 80°C. The final temperature of the mixture is 40°C
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A block of ice of mass $120\, g$ at temperature $0^{\circ} C$ is put in $300\, gm$ of water at $25^{\circ} C$ The $xg$ of ice melts as the temperature of the water reaches $0^{\circ} C$ The value of $x$ is [Use: Specific heat capacity of water $=4200\,Jkg ^{-1} K ^{-1}$, Latent heat of ice = 3.5 \(\times\) 105 JKg-1]
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- The water equivalent of a calorimeter is $10\, g$ and it contains $50 \,g$ of water at $15�C$. Some amount of ice, initially at $-10�C$ is dropped in it and half of the ice melts till equilibrium is reached. What was the initial amount of ice that was dropped (when specific heat of ice $= 0.5 \,cal\, gm^{-1}�C^{-1},$ specific heat of water $= 1.0 \,cal\, gm^{-1}�C^{-1}$ and latent heat of melting of ice $= 80 \,cal \,gm^{-1}$) ?
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- One kilogram of ice at $0^{\circ} C$ is mixed with one kilogram of water at $80^{\circ} C$. The final temperature of the mixture is (Take specific heat of water $=4200\, kJ / kg -{ }^{\circ} C$, Latent heat of ice $=336\, kJ / kg$ )
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Concepts Used:
Calorimetry
In chemistry and thermodynamics, calorimetry is the science or act of measuring changes in state variables of a body for the purpose of deriving the heat transfer associated with changes of its state due, for example, to chemical reactions, physical changes, or phase transitions under specified constraints. Calorimetry is performed with a calorimeter. Scottish physician and scientist Joseph Black, who was the first to recognize the distinction between heat and temperature, is said to be the founder of the science of calorimetry.
Calorimeter Principle
When two bodies of different temperatures (preferably a solid and a liquid) are placed in physical contact with each other, the heat is transferred from the body with higher temperature to the body with lower temperature until thermal equilibrium is attained between them. The body at higher temperature releases heat while the body at lower temperature absorbs heat. The principle of calorimetry indicates the law of conservation energy, i.e. the total heat lost by the hot body is equal to the total heat gained by the cold body.
The heat transfer in a system is calculated using the formula,
Heat Lost = Heat Gained
Where
q is the measure of heat transfer
m is the mass of the body
c is the specific heat of the body
Δt is the change in the temperature