Thermodynamics - Apple

Graph of ice to water to steam.
In the above graph, a block of ice starts at a temperature below
the melting point of water (cold ice). The first line segment is the
temperature change of the ice from -20° C to 0° C. The first
horizontal segment is the ice melting. The heat source does not
raise the temperature, it is just melting the ice. Once the ice is
melted the heat source is causing the water to increase in
temperature. At 100° C the water boils. It does not change
temperature it just boils into steam. If we capture the steam and
continue to add heat the temperature of the steam will increase.
Of course the gas laws will then become part of the equation.
The energy required to melt ice is called the heat of fusion and
is 335 J/g (that's gram) or 3.35 x 10 5 J/kg. The energy
required to turn water to steam is called the heat of
vaporization is 2260 J/g or 2.26 x 10 6 J/kg.
21. How much energy is required to melt 15.3 g of ice?
22. How much energy is required to change 2.7 g of water at
100C to steam?
23. What energy is required to raise a 5 g ice cube at -12°C to
water at 17°C? (three parts, heat the ice, melt the ice, heat the
water)
24. How much energy is required to raise 37 g of water at 17°C
to steam at 141°C?
25. A 17 g ice cube at -11°C is placed on a 135 g slab of
aluminum at 71°C. What is the final temperature after everything
comes to equilibrium? Assume all the ice melts.
26. A 2.0 kg block of silver at 70°C is placed on a large block of
ice at 0°C. When equilibrium is reached, how much ice is
melted?
27. 3.0 g of steam at 130°Care admitted to a 440 g steel
container at 20°C. What is the temperature of the water when
equilibrium is reached?
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