Advertisements
Advertisements
Question
63.2 g of copper at 50°C can just melt 3.8g of ice. If the specific latent heat of ice is 336 J/g, find the specific heat capacity of copper.
Advertisements
Solution
Let the specific heat capacity of copper be s
∴ Heat lost by copper = 63.2 × s × (50 - 0) = 3160 s joule
Heat gained by ice = 3.8 × 336 joule
Since Heat gained = Heat lost
We have 3160s = 3.8 × 336 = 1276.8
Or s = (1276.8/3160) K/g °C = 0.404 J/g °C.
RELATED QUESTIONS
It is generally cold after a hail-storm then during and before the hail storm. Give reason.
Indian style of cooling drinking water is to keep it in a pitcher having porous walls. Water comes to the outer surface very slowly and evaporates. Most of energy needed for evaporation is taken from the water itself and the water is cooled down. Assume that a pitcher contains 10 kg of water and 0.2 g of water comes out per second. Assuming no backward heat transfer from the atmosphere to the water, calculate the time in which the temperature decrease by 5°C. Specific heat capacity of water = 4200 J kg−1 °C−1 and latent heat of vaporization of water = 2.27 × 106 J kg−1.
The substances like water which have ........... Heat capacity warm up more slowly than substances like iron which have .......... heat capacity.
What are other units of heat? Name and define them.
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’.
- Where does heat transfer take place?
- In such a situation which principle of heat do you perceive?
- How can this principle be explained in short?
- Measuring the property of which substance this principle is used?
Derive Meyer’s relation for an ideal gas.
For a gas `"R"/"C"_"v" = 0.4,` where 'R' is the universal gas constant and 'Cv' is molar specific heat at constant volume. The gas is made up of molecules which are ______.
A piece of lead weighing 500 g gives out 1200 calories of heat when it is cooled from 100° C to 20° C. Find its specific heat.
A metal ball of heat capacity 50J/°C loses 2000 J of heat. By how much will its temperature fall?
