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Latent heat and energy during a phase transition

A 50.0 gram ice cube at -2 oC is heated until all of it is turned to steam at 100.0 oC. How much energy in calories was added to do this?

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Solution Preview

Please see the attached file.

Step 1: Convert all temp in to the Kelvin scale or Absolute scale by adding 273
Step 2: Convert all units to SI system ie: 50 gm =0.05Kg.
Answer to your problem
Consider 50 gm = 0.05 kg of ice at a temperature toC below the normal melting point of ice is converted to the normal melting point of ice = 273 K. Let it is gradually heated, and converted to steam at 100oC or 373K. The total change in energy during the process
which follows

a. The Quantity of heat dQ to be supplied to it so that its temperature if ice rises by dT ( from 271 K to 273 K)

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Solution Summary

The problem describes the change in energy during a first order phase transition. The transition from ice to water and water to steam required energy. This example beautifully explains this process.

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