At 1 atm, how much energy is required to heat 39.0 g of H2O(s) at –16.0 °C to H2O(g) at 159.0 °C? Helpful constants can be found here.
Ti = -16.0
Tf = 159.0
here
Cs = 2.09 J/goC
Heat required to convert solid from -16.0 oC to 0.0 oC
Q1 = m*Cs*(Tf-Ti)
= 39 g * 2.09 J/goC *(0--16) oC
= 1304.16 J
Lf = 333.0 J/g
Heat required to convert solid to liquid at 0.0 oC
Q2 = m*Lf
= 39.0g *333.0 J/g
= 12987 J
Cl = 4.184 J/goC
Heat required to convert liquid from 0.0 oC to 100.0 oC
Q3 = m*Cl*(Tf-Ti)
= 39 g * 4.184 J/goC *(100-0) oC
= 16317.6 J
Lv = 2260.0 J/g
Heat required to convert liquid to gas at 100.0 oC
Q4 = m*Lv
= 39.0g *2260.0 J/g
= 88140 J
Cg = 2.03 J/goC
Heat required to convert vapour from 100.0 oC to 159.0 oC
Q5 = m*Cg*(Tf-Ti)
= 39 g * 2.03 J/goC *(159-100) oC
= 4671.03 J
Total heat required = Q1 + Q2 + Q3 + Q4 + Q5
= 1304.16 J + 12987 J + 16317.6 J + 88140 J + 4671.03 J
= 123419.79 J
= 123.4 KJ
Answer: 123.4 KJ
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