How much heat in Joules would it take to melt 2.45 g of ice at 0.0OC and then raise the temperature of the water to 75.0OC?

Question

A- 820 J

B- 768 J

C- 1000 J

D- 1588 J

Answer 1

Step 1: melt 2.45 g of ice @ 0ºC (phase change, no change in temperature)

q = m∆Hfusion = (2.45 g)(334 J/g) = 818 J

Step 2: raise temperature of 2.45 g liquid water from 0º to 75º

q = mC∆T = (2.45 g)(4.184 J/gº)(75º) = 769 J

Add q from steps 1 and 2:

818 J + 769 J = 1587 J so answer (D) would be correct