In: Chemistry
calculate the amount of J required to heat 115.0g of solid H2O at -25 degrees C to liquid H20 at 30 degrees C
-25 oC ------------------> 0 oC----------------------> 30oC
(1) (2) (3)
there are 3 energy conversions
Q = Q1 + Q2 + Q3
Q1 = m Cp dT
Q1 =115 x 2.09 x 25
Q1 = 6009 J
moles of soldi = 115 / 18 = 6.39
Q2 = n x delta H fusion = 6.39 x 6.01 x 10^3
= 38397 J
Q3 = m Cp dT
Q3 = 115 x 4.184 x 30
Q3 = 14435 J
Q = Q1 + Q2 + Q3
Q = 58841 J
amount of heat required = 58841 J