Question

How much heat (in KJ) is required to warm 13.0 g of ice, initially at -10.0...

How much heat (in KJ) is required to warm 13.0 g of ice, initially at -10.0 *C, to steam at 113.0 degress C? The heat capacity of ice is 2.09 J/g degress C and that of steam is 2.01 J/g * C. Show work.

Q = heat change for conversion of ice at -10 oC to ice at 0 oC + heat change for

conversion of ice at 0oC to water at 0oC + heat change for conversion of water at 0oC to water at 100 oC +heat change for conversion of water at 100 oC to vapour at 100 oC+ heat change for conversion of vapour at 100 oC to vapour at 113 oC

Amount of heat required , Q = mcdt + mL + mc'dt + mL' + mc"dt"

= m(cdt + L + c'dt' + L' + c"dt" )

Where

m = mass of ice = 13.0 g

c'' = Specific heat of steam = 2.01 J/g degree C

c' = Specific heat of water = 4.186 J/g degree C

c = Specific heat of ice= 2.09 J/g degree C

L’ = Heat of Vaporization of water = 2260 J/g

L= Heat of fusion of ice = 334.9 J/g

dt’’ = 113-100 = 13oC

dt' = 100 -0 =100 oC

dt = 0-(-10)=10 oC

Plug the values we get Q = m(cdt + L + c'dt '+ L' + c"dt" )

= 39.8 x103 J

= 39.8 kJ

Therefore the amount of heat required is 39.8 kJ