A 0.580kg chunk of an unknown metal that has been in boiling water for several m

Question

A 0.580kg chunk of an unknown metal that has been in boiling water for several minutes is quickly dropped into an insulating StyrofoamTM beaker containing 1.22kg of water at room temperature (20.2?C). After waiting and gently stirring for 5.00 minutes, you observe that the water's temperature has reached a constant value of 22.1?C.

Part A

Assuming that the StyrofoamTM absorbs a negligibly small amount of heat and that no heat was lost to the surroundings, what is the specific heat capacity of the metal?

Part B

Which is more useful for storing energy from heat, this metal or an equal weight of water? Explain.

Which is more useful for storing energy from heat, this metal or an equal weight of water? Explain.

Part C

What if the heat absorbed by the StyrofoamTM actually is not negligible. How would the specific heat capacity you calculated in part A be in error? Would it be too large, too small, or still correct?

What if the heat absorbed by the StyrofoamTM actually is not negligible. How would the specific heat capacity you calculated in part A be in error? Would it be too large, too small, or still correct?

Explanation / Answer

Part A)
By conservation of energy

Q = Q, thus mc(delta T) = mc(delta T)

(.580)(c)(77.9) = (1.22)(4186)(1.9)

c = 214.8 J/Kg C

Part B)

Water has a much larger value of c so stores more heat for the same ?T.

Part C)

If some of the heat went into the StyrofoamTM then more would have to come out of the metal and c would be found to be greater. The value calculated in A would be too small.

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