14.Calculate the quantity of heat required to raise the temperature of 10g of ice
from −10°C to steam 110°C and draw the graph of Temperature (°c) versus
Heat (Joule or Cal.)
To calculate the quantity of heat required, we need to consider the different phases of water and the specific heat capacities associated with each phase.
1. Heating ice from -10°C to 0°C:
Q = m * c * ΔT
Q = 10g * 2.09 J/g°C * 10°C
Q = 209 J
2. Melting ice at 0°C:
Q = m * Lf
Q = 10g * 334 J/g
Q = 3340 J
3. Heating water from 0°C to 100°C:
Q = m * c * ΔT
Q = 10g * 4.18 J/g°C * 100°C
Q = 4180 J
4. Vaporizing water at 100°C:
Q = m * Lv
Q = 10g * 2260 J/g
Q = 22600 J
5. Heating steam from 100°C to 110°C:
Q = m * c * ΔT
Q = 10g * 2.01 J/g°C * 10°C
Q = 201 J
Total heat required = 209 J + 3340 J + 4180 J + 22600 J + 201 J
= 30230 J
Now, let's draw the graph of Temperature (°c) versus Heat (Joule or Cal.):
Temperature (°C) Heat (Joules)
-10 0
0 209
0 3549
100 7729
100 30329
110 30530
The graph will show a linear increase in heat as the temperature of the ice increases, with significant increases at the phase changes from solid to liquid and liquid to gas.