A sample containing 1200.0 grams of ice at -13.8°C is given 580.0 kJ of heat. ΔHfusion = 6.01 kJ/mol ΔHvap = 40.8 kJ/mol Specific heat of ice = 1.877 J/gK Specific heat of water = 4.184 J/gK Specific heat of steam = 2.013 J/gK. How much energy (in kJ) is needed to heat the 1200.0 grams of ice up to 0.00°C? How much energy (in kJ) is needed to melt 1200.0 grams of ice at 0.00°C to water at 0°C? How much energy (in kJ) is needed to heat the 1200.0 grams of water from 0.00°C to the boiling point of water?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
A sample containing 1200.0 grams of ice at -13.8°C is given 580.0 kJ of heat.
ΔHvap = 40.8 kJ/mol
Specific heat of ice = 1.877 J/gK
Specific heat of water = 4.184 J/gK
Specific heat of steam = 2.013 J/gK.
How much energy (in kJ) is needed to heat the 1200.0 grams of ice up to 0.00°C?
How much energy (in kJ) is needed to melt 1200.0 grams of ice at 0.00°C to water at 0°C?
How much energy (in kJ) is needed to heat the 1200.0 grams of water from 0.00°C to the boiling point of water?
If you start at -13.8°C, what is the final temperature of the system after you have added the 580.0 kJ of heat? (in °C)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
