Question
How much total heat is required to heat 3316 g of ice at -16.12 oC to all steam at a temperature of 128.08 oC?
how do you carry out the five step process?
how do you carry out the five step process?
Answers
Gibbons
Heat needed to raise the temperature of ice from -16.12c to 0c=mcT
=3.316*2100*16.12
=112253.23 joules
Heat to melt the ice=mL
=3.316*336000
=1114176 joules
Heat needed to raise the temperature of the water from 0c to 100c=mcT
=3.316*4200*100
=1392720 joules
Heat needed to vaporise 3.316kg of water=mL
=3.316*2260000
=7494160 joules
Heat needed to raise the temperature of steam from 100c to 128.8c=mcT
=3.316*2100*28.8
=200551.68 joules
Total heat required= 112253.23+1114176+1392720+7494160+200551.68
=10313860 joules
=3.316*2100*16.12
=112253.23 joules
Heat to melt the ice=mL
=3.316*336000
=1114176 joules
Heat needed to raise the temperature of the water from 0c to 100c=mcT
=3.316*4200*100
=1392720 joules
Heat needed to vaporise 3.316kg of water=mL
=3.316*2260000
=7494160 joules
Heat needed to raise the temperature of steam from 100c to 128.8c=mcT
=3.316*2100*28.8
=200551.68 joules
Total heat required= 112253.23+1114176+1392720+7494160+200551.68
=10313860 joules