Question 14
[11]
14.1
Define the specific heat capacity of a substance.
(2)
14.2
A small object of mass m = 250 g and unknown specific heat capacity c, initially
at 100 °C, is placed into a body of liquid with a heat capacity of 1300J K~, initially
at 20 °C. The final equilibrium temperature is 27 °C. What is the value of c?
Ignore any heat that may be absorbed by the vessel containing the liquid.
(4)
14.3
154 g of crushed ice at -20° C is removed from a freezer and placed ina
calorimeter. Thermal energy is supplied to the ice at a constant rate of 530 W.
To ensure that all the ice is at the same temperature, it is continually stirred.
The temperature of the contents of the calorimeter is recorded every 15 seconds.
Figure 3 below shows the variation with time t of the temperature @ of the
contents of the calorimeter.
A/°C
0
25
50
75
100
125
150
175
200
tls
Figure 3
14.3.1 Determine the specific heat capacity of ice.
(3)
14.3.2 Determine the specific latent heat of fusion of ice.
(2)
Question 15
[10]
15.1
List four assumptions of the kinetic model of ideal gases.
(4)
15.2
An ideal gas is kept in a cylinder by a piston that is free to move. The gas is
heated such that its internal energy increases and the pressure remains constant.
Use molecular model of ideal gases to explain the increase in internal energy. (2)
15.3
A cylinder contains 50 L of argon gas at 18.4 atm and 127 °C. How many moles
of argon gas is in the cylinder?
(2)
15.4 The volume of the cylinder is decreased by a half at a constant temperature,
what is the new pressure of argon gas in atm and in Pa?
(2)
THE END
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