Calculate the change in heat when 17.0 g of water vapor (steam) at 100.0°C condenses to liquid water and then cools to 22.5 °C
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A patient arrives in the emergency room with a burn caused by steam. Calculate the heat that is released when 17.4 g of steam at 100. âC hits the skin, condenses, and cools to body temperature of 37.0 âC. (For water, 540 cal (2260 J) is needed to convert 1 g of water to vapor at 100 âC.)
Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following:
A. joules needed to melt 90.0 g of ice at 0 âC and to warm the liquid to 85.0
B. kilocalories released when 30.0 g of steam condenses at 100 âC and the liquid cools to 0 âC
C. kilojoules needed to melt 26.0 g of ice at 0 âC, warm the liquid to 100 âCand change it to steam at 100 âC
âC
Calculate the change in heatwhen 12.60g of water vapor (steam) at 100.0C condenses to liquidwater and then cools to 22.50C. For water:
Sice=2.09J/g*C
DeltaHfus=6.01kJ/mol
Swater=4.184J/g*C
DeltaHvap=40.79kJ/mol
Ssteam=1.99J/g*C
Every time i work it out i getit wrong, I keep getting 34721 Joules as the answer, Thankyou