A 50 g copper calorimeter contains 250 g of water at 20 C. How much steam be condensed into the water to make the final temperature of the system 50 C. ( specific heat water= 4200 J/Kg C , specific heat copper= 390 J/Kg C

Approximately of steam at (assuming that the boiling point of water in this experiment is .)

Explanation:

Latent heat of condensation/evaporation of water: .

Both mass values in this question are given in grams. Hence, convert the specific heat values from this question to .

Specific heat of water: .

Specific heat of copper: .

The temperature of this calorimeter and the of water that it initially contains increased from to . Calculate the amount of energy that would be absorbed:

.

.

Hence, it would take an extra of energy to increase the temperature of the calorimeter and the of water that it initially contains from to .

Assume that it would take grams of steam at ensure that the equilibrium temperature of the system is .

In other words, of steam at would need to release as it condenses (releases latent heat) and cools down to .

Latent heat of condensation from of steam: .

Energy released when that of water from the steam cools down from to :

.

These two parts of energy should add up to . That would be exactly what it would take to raise the temperature of the calorimeter and the water that it initially contains from to .

.

Solve for :

.

Hence, it would take approximately of steam at for the equilibrium temperature of the system to be .

heat the gas and measure the pressure

the displacement produced by the body.  

the amount of force subjected to the body.  

the angle between the direction of force and displacement