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.
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
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves. Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Ihrig's class at Green River Community College.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.