# Problem: From the data below, calculate the total heat (in J) needed to convert 22.00 g of ice at −6.00°C to liquid water at 0.500°C: mp at 1 atm:     0.0°C                      Δ  H°fus:      6.02 kJ/molcliquid:               4.21 J/g•°C              csolid:        2.09 J/g•°C

###### FREE Expert Solution

We’re being asked to calculate the amount of total heat (in J) needed to convert 22.00 g of ice at −6.00°C to liquid water at 0.500°C:

Note that cooling and freezing is an exothermic process, which means q is negative (–)

There are two heats involved in this problem:

1. q1 which is the heat in heating 22 g of ice from -6˚C to 0 ˚C

2. q2 which is the heat in melting 22 g of ice at 0 ˚C

3. q3 which is the heat in heating 22 g of water from 0˚C to 0.5 ˚C

We need to solve for each heat individually then add them together to get the final answer.

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###### Problem Details

From the data below, calculate the total heat (in J) needed to convert 22.00 g of ice at −6.00°C to liquid water at 0.500°C:

mp at 1 atm:     0.0°C                      Δ  H°fus:      6.02 kJ/mol
cliquid:               4.21 J/g•°C              csolid:        2.09 J/g•°C