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?© BrainMass Inc. brainmass.com October 24, 2018, 7:52 pm ad1c9bdddf
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
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)
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.
Heat Required for Phase Conversion
The fluorocarbon C2Cl3F3 has a normal boiling point of 47.6 degrees C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91J/g-K and 0.67J/g-L, respectively. The heat of vaporization for the compound is 27.49kj/mol. I need to find the heat required to convert 25.0g of C2Cl3F3 from a liquid at 5.00 degrees C to a gas at 82.00 degreesC. Could you please show all steps and conversions so I understand it better.
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