A cooler contains 1 kg of ice at -5°C. 2 kg of water at 50°C is
added to the cooler. If the cooler does not exchange any heat with
the rest of the world, what is the final temperature of the ice and
water?
A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of
water in an 80-g aluminum container, both
initially at 30°C. What is the final equilibrium temperature?
(Specific heat for aluminum is 900 J/kg×°C,
the specific heat of water is 4 186 J/kg×°C, and
Lf = 3.33 ´ 105 J/kg.)
A 50·g ice cube (at 0°C) is placed in an insulated cup with
250·g of water which is at 46°C. The latent heat of fusion for ice
is 80·cal/g and the specific heat of water is 1.0·cal/g/°C.
(a) How much heat will the ice have to absorb from the water to
completely melt (and turn into 0°C water)? ___ cal.
(b) Find the temperature of the 250·g of water initially at 46°C
after it loses the heat required to melt...
How much heat is evolved in converting 1.00 mol of steam at
160.0 ∘C to ice at -55.0 ∘C? The heat capacity of steam is 2.01
J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C). Express your answer in units
of kilojoules Assume the system is at atmospheric pressure.
How much heat is evolved in converting 1.00 mol of steam at
140.0 ∘C to ice at -45.0 ∘C? The heat capacity of steam is 2.01
J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).
How much heat is evolved in converting 1.00 mol of steam at
135.0 ∘C to ice at -55.0 ∘C? The heat capacity of steam is 2.01
J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).
How much heat is evolved in converting 1.00 mol of steam at
130.0 ∘C to ice at -50.0 ∘C? The heat capacity of steam is 2.01
J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).
How much heat is evolved in converting 1.00 mol of steam at
150.0 ∘C to ice at -45.0 ∘C? The heat capacity of steam is 2.01
J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).
How much heat is evolved in converting 1.00 mol of steam at
160.0 ∘C to ice at -50.0 ∘C? The heat capacity of steam is 2.01
J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).