A 4.00 kg iron pan at 225degreeC is put into a sink of water initially at 45.0de

Question

A 4.00 kg iron pan at 225degreeC is put into a sink of water initially at 45.0degreeC. If the final temperature of the water is 55.0degreeC then how much water is in the sink assuming heat loss to the surroundings is negligible (C_ion= 0.106 cal g idegreeC-1)? A heat engine with 35% efficiency (remarkable...) performs 2550 J of work. (a)How much heat is absorbed from the burning fuel (Q_c) and how much heat is released to the environment (Qc)? if the temperature of the surroundings is 290 K then what must the temperature (T_a) of the burning fuel be? if 1250 J of heat are irreversibly transferred directly from a hot reservoir at800. K to a cokl reservoir at 350. K then what is the change in entropy of the universe? if an ideal, reversible engine is placed between the two energy reservoirs of part (a) then what is the maximum work that can be done? State whether your result indicate a decrease, increase or no change in the disorder of the universe. For a reversible process is Del S_univ greater than, equal to or less than zero? Does this mean the randomness of the universe increases, decreases or stays the same? For an irreversible process is Del S_univ, greater than, equal to. or less than zero? Does this mean the randomness of the universe increases, decreases or stays the same?

Explanation / Answer

(1).Mass of iron m = 4 kg = 4000 g

Initial temprature of iron t = 225 o C

Mass of water M = ?

Initial temprature of water t ' = 45 o C

Final temprature of water T = 55 o C

Specific heat of iron C = 0.106 cal / g oC

Specific heat of water C ' = 1 cal / g oC

Heat lost by iron = Heat gain water

mC(t -T) = MC ' (T - t ')

4000(0.106)(225-55) = M(1)(55-45)

72080 = 10 M

      M = 7208 g

          = 7.208 kg

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