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In Regnault'S Apparatus for Measuring Specific Heat Capacity of a Solid, There is an Inlet and an Outlet in the Steam Chamber. the Inlet is Near the Top and the Outlet is Near the Bottom.

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प्रश्न

In Regnault's apparatus for measuring specific heat capacity of a solid, there is an inlet and an outlet in the steam chamber. The inlet is near the top and the outlet is near the bottom. Why is it better than the opposite choice where the inlet is near the bottom and the outlet is near the top?

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उत्तर

The inlet is near the top and the outlet is near the bottom because there is a loss of heat from the steam as it passes through the chamber. As the steam loses heat, a part of it condenses back to water and the cold steam gets denser and moves down towards the bottom.

But when done the other way round, the used steam does not pass through the chamber correctly and gets mixed up. This can result in discrepancy in the desired results.

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पाठ 25: Calorimetry - Short Answers [पृष्ठ ४६]

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एचसी वर्मा Concepts of Physics Volume 1 and 2 [English]
पाठ 25 Calorimetry
Short Answers | Q 5 | पृष्ठ ४६

संबंधित प्रश्‍न

In an experiment on the specific heat of a metal, a 0.20 kg block of the metal at 150 °C is dropped in a copper calorimeter (of water equivalent 0.025 kg) containing 150 cm3 of water at 27 °C. The final temperature is 40 °C. Compute the specific heat of the metal. If heat losses to the surroundings are not negligible, is your answer greater or smaller than the actual value for the specific heat of the metal?


Given below are observations on molar specific heats at room temperature of some common gases.

Gas

Molar specific heat (Cv)

(cal mol–1 K–1)

Hydrogen 4.87
Nitrogen 4.97
Oxygen 5.02
Nitric oxide 4.99
Carbon monoxide 5.01
Chlorine 6.17

The measured molar specific heats of these gases are markedly different from those for monatomic gases. Typically, molar specific heat of a monatomic gas is 2.92 cal/mol K. Explain this difference. What can you infer from the somewhat larger (than the rest) value for chlorine?


Define heat capacity and state its SI unit.


Calculate the mass of ice needed to cool 150 g of water contained in a calorimeter of mass 50 g at 32 °C such that the final temperature is 5 °C. Specific heat capacity of calorimeter = 0.4 J g-1 °C-1, Specific heat capacity of water = 4.2 J g-1°C-1, latent heat capacity of ice = 330 J g-1.


A copper vessel of mass 100 g contains 150 g of water at 50°C. How much ice is needed to cool it to 5°C?

Given: Specific heat capacity of copper = 0.4 Jg-1 °C-1

The Specific heat capacity of water = 4.2 Jg-1 °C-1

The Specific latent heat of fusion ice = 336 Jg-1


Name a liquid which has the highest specific heat capacity.


Write the approximate value of specific heat capacity of water in S.I. unit.


Give one example where high specific heat capacity of water is used as heat reservoir ?


A mass m1 of a substance of specific heat capacity c1 at temperature t1 is mixed with a mass m2 of other substance of specific heat capacity c2 at a lower temperature t2. Deduce the expression for the temperature t of the mixture. State the assumption made, if any.


In an experiment to determine the specific heat capacity of a solid following operations were
made:
Mass of calorimeter + stirrer = x kg
Mass of water = y kg
Initial temperature of water t1℃
Mass of solid = z kg
Temperature of solid = t2 ℃
Temperature of mixture = t ℃
Specific heat capacity of calorimeter and water are c1 and c2 respectively. Express the specific
heat capacity c of the solid in terms of the above data.


An electric heater of power 600 W raises the temperature of 4.0 kg of a liquid from 10.0℃ to 15.0℃ in100 s. Calculate:

  1. the heat capacity of 4.0 kg of liquid,
  2. the specific heat capacity of the liquid.

Ice cream appears colder to the mouth than water at 0℃. Give reason.


How will rise in sea level affect population in coastal countries?


How will climate changes affect the various animal species?


Who shall pay carbon tax ?


(i) State whether the specific heat capacity of a substance remains the same when its state changes from  solid to liquid. 
(ii) Give one example to support your answer.


104g of water at 30°C is taken in a calorimeter made of copper of mass 42 g. When a certain mass of ice at 0°C is added to it, the final steady temperature of the mixture after the ice has melted, was found to be 10°C. Find the mass of ice added. [Specific heat capacity of water = 4.2 Jg–1°C–1 ; Specific latent heat of fusion of ice = 336 Jg–1; Specific heat capacity of copper = 0.4 Jg–1°C–1] .


Write the SI unit of specific heat.

A liquid X has specific heat capacity higher than the liquid Y. Which liquid is useful as coolant in car radiators.


m kg of a substance of specific heat capacity s J/kg °C is heated so that its temperature rises from θ1°C to θ2°C. Write down the expression for the heat Q supplied.


Is it possible to condense the water formed, back to ice by adding ice at 0°C. Explain with reason.


Ice-cream at 0°C feels colder than water at 0°C. Give reason for this observation.


A vessel of negligible heat*capacity contains 40g of ice in it at 0°C, 8g of steam at 100°C is passed into the ice to melt it. Find the final temperature of the contents of the vessel.
(Specific latent heat of vaporization of steam = 2268 J/g, specific latent heat of fusion of ice = 336 J/f and specific heat capacity of water = 4.2 J/g°C)


Derive an expression for finding out the specific heat capacity of a body (solid) from the readings of an experiment given below:

(i) Mass of empty calorimeter (with stirrer) = m1 gm

(ii) Mass of the metal piece = M gm

(iii) Mass of colorimeter and water = m2 gm

(iv) Initial temperature and water = t1°C

(v) Temperature of hot solid (metal piece) = t2 °C

(vi) Final temperature of the mixture = t°C

(vii) Specific heat of calorimeter = 0.4 J gm / °C


How much heat energy is necessary to raise the temperature of 5 kg of water from 20°C to 100°C?


Read the passage and answer the questions based on it.

If heat is exchanged between a hot and cold object, the temperature of the cold object goes on increasing due to gain of energy and the temperature of the hot object goes on decreasing due to loss of energy. The change in temperature continues till the temperatures of both objects attain the same value. In this process, the cold object gains heat energy and the hot object loses heat energy. If the system of both the objects is isolated from the environment by keeping it inside a heat-resistant box then no energy can flow from inside the box or come into the box. In this situation, we get the following principle.
Heat energy lost by the hot object = Heat energy gained by the cold object. This is called the ‘Principle of heat exchange’.

  1. Where does heat transfer take place?
  2. In such a situation which principle of heat do you perceive?
  3. How can this principle be explained in short?
  4. Measuring the property of which substance this principle is used?

_______ is defined as the amount of heat required to raise the temperature of 1kg of a substance by 1°C.


When a uniform rod is heated, which of the following quantity of the rod will increase


For a gas, `"R"/"C"_"v"=0.4`, where R Is universal gas constant and Cv is the molar specific heat at constant volume. The gas is made up of molecules, which are ______


If 'Cp' and 'Cv' are molar specific heats of an ideal gas at constant pressure and volume respectively. If 'λ' is the ratio of two specific heats and 'R' is universal gas constant then 'Cp' is equal to ______.


50 g of copper is heated to increase its temperature by 10° C. If the same quantity of heat is given to 5 g water, the rise in its temperature is [Specific heat of copper = 420 joule-kg-1 °C-1 , specific heat of water = 4200 joule-kg-I °C-1]


Which of the following substances (A, B and C) has the highest specific beat?


Conductors have generally high specific heat capacities and insulators have low specific heat capacities.


To study energy exchange between hot and cold objects, the system of both objects is isolated from the environment by keeping them inside ______.


A block of ice of mass 120 g at temperature 0°C is put in 300 gm of water at 25°C. The xg of ice melts as the temperature of the water reaches 0°C. The value of x is ______.

[Use: Specific heat capacity of water = 4200 Jkg-1K-1, Latent heat of ice = 3.5 × 105 Jkg-1]


In the method of mixtures, a hot metal is dropped into cold water and the mixture reaches a final temperature. Which principle is used to find the specific heat of the metal?


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