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Question

i cant get the correct answer for this problem. What is it and how do you get it.


How much heat in kilojoules is required to warm 12.4 g of ice, initially at -10.0°C, to steam at 110.0°C? The heat capacity of ice is 2.09 J/g °C and that of steam is 1.84 J/g °C.
_____kJ

Answer 1

You are not providing all the info.

1.You have an amount of energy required to heat the ice from -10 to ice at 0 deg: Q1=m*C(ice)*ΔT= 12.4*2.09*0.001*(0-(-10) = 0.259 kJ
2. You need to give the latent heat (0.334kJ/g) so that ice at 0 deg becomes liquid water and 0 deg: Q2=0.334*m= 0.334*12.4=4.142 kJ
3.You need to give energy to go from liquid water at 0 deg to liquid water at 100 deg.: Q3= m*C(water)*ΔT =12.4*4.184*0.001*(100-0) =5.188 kJ
4. You need to give the latent heat (2.272 KJ/g) so that water at 100 deg becomes steam at 100 deg: Q4=2.272*m= 2.272*12.4 = 28.173
5. You need to give energy to fo from steam at 100 deg to steam at 110 deg : Q5=mC(steam)ΔT= 12.4*1.84*0.001*(110-100)= 0.228

So the total amount is
Q= Q1 + Q2 + Q3+ Q4 + Q5 =37.99 kJ

Please check for numerical errors