Section 6: Multi-Step Heat Calculation How much heat energy is needed to heat 62.3 g of ice from -30.0°C to 95.0°C? Cp ice = 2.09 J/g°C AHfus =6.01 kJ/mol Cp water = 4.18 J/g°C Step 1: Step 2: Step 3: Total amount of heat needed:

Section 6: Multi-Step Heat Calculation How much heat energy is needed to heat 62.3 g of ice from -30.0°C to 95.0°C? Cp ice = 2.09 J/g°C AHfus =6.01 kJ/mol Cp water = 4.18 J/g°C Step 1: Step 2: Step 3: Total amount of heat needed:

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.49PAE: 9.49 Hvap=31.3 kJ/mol for acetone. If 1.40 kg of water were vaporized to steam in a boiler, how much...

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Concept explainers

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.

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Section 6: Multi-Step Heat Calculation
How much heat energy is needed to heat 62.3 g of ice from -30.0°C to 95.0°C?
Cp ice =2.09 J/g°C
AHfus =6.01 kJ/mol
Cp water = 4.18 J/g°C
Step 1:
Step 2:
Step 3:
Total amount of heat needed:
d it

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