Calculate Energy Needed to Heat 4.6 kg Water

AI Thread Summary
To calculate the energy needed to heat 4.6 kg of ice from 0 degrees Celsius to vapor at 106 degrees Celsius, multiple equations are required. The process involves four distinct steps: first, calculating the energy to melt the ice into liquid water; second, determining the energy needed to raise the temperature of the liquid water to 100 degrees Celsius; third, calculating the energy to evaporate the water into vapor; and finally, finding the energy required to raise the vapor to 106 degrees Celsius. Each step utilizes specific formulas: Q = mcΔt for temperature changes, Q = ml_f for phase changes from solid to liquid, and Q = ml_v for phase changes from liquid to vapor. Summing the energy from all four parts provides the total energy required for the entire heating process.
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Determine the energy needed to raise the temperature of 4.6 of 0 degrees celsius ice to 106 degrees celsius vapour given the values for water: 5 marks
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l[subscript]f= 333kJ/kg, l[subscript]v = 2255 kJ, c[subscript]liquid = 4200 J/kg c[subscript]vapour = 2000 J/Kg degrees celsius
I just have one question, do you need all these equations?:
Q = mc[delta]t, Q = ml[subscript]f Q=ml[subscript]v
and basically add them all up?
 
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yup, that's right
 
I can tell you that it is a four part question.

A) Energy to melt the solid ice.
B) Energy to raise liquid to 100.
C) Energy to evaporate into vapor.
D) Energy to raise vapor to 106.
 
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