Need to solve this Calorimetry problem.
-
q = ms(change T)
q1 = (161 g)(4.184 J/g*C)(85)
q1 = 57258.04 Joules from 85 C to 0 C
At 0 C we have a phase change.
161 g x 1 mol/18.106 g = 8.94 mols H2O
q2 = (8.94 mols)(6.01 kJ/mol) = 53.7294 kJ
Add q1 and q2 (don't forget to convert q1 to kJ!)
57.25804 kJ + 53.7294 kJ = 111 kJ
q1 = (161 g)(4.184 J/g*C)(85)
q1 = 57258.04 Joules from 85 C to 0 C
At 0 C we have a phase change.
161 g x 1 mol/18.106 g = 8.94 mols H2O
q2 = (8.94 mols)(6.01 kJ/mol) = 53.7294 kJ
Add q1 and q2 (don't forget to convert q1 to kJ!)
57.25804 kJ + 53.7294 kJ = 111 kJ