Datasheet Part 2 mass of empty cups, g 2.11716 mass of cups+100 mL water, g 102.3718 mass of warm water, g 100.25464 mass of ice added, g 25.4224 initial temperature of warm water, C 37.55 final temperature of warm water + melted ice, C 29.8 initial temperature of ice 0 mass of water in calorimeter (final), g 125.67704 ΔH warm water J ΔH ice water J ΔH fusion J ΔH fusion per gram of ice J/g ΔH fusion per mole of ice J/mol ΔH fusion per mole of ice kJ/mol accepted ΔH fusion per mole of ice 6.01 kJ/mol % error Need some help solving this table. the answer I came up with seemed like it was way off. Can someone help?
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.
| Datasheet Part 2 | ||
| mass of empty cups, g | 2.11716 | |
| mass of cups+100 mL water, g | 102.3718 | |
| mass of warm water, g | 100.25464 | |
| mass of ice added, g | 25.4224 | |
| initial temperature of warm water, C | 37.55 | |
| final temperature of warm water + melted ice, C | 29.8 | |
| initial temperature of ice | 0 | |
| mass of water in calorimeter (final), g | 125.67704 | |
| ΔH warm water | J | |
| ΔH ice water | J | |
| ΔH fusion | J | |
| ΔH fusion per gram of ice | J/g | |
| ΔH fusion per mole of ice | J/mol | |
| ΔH fusion per mole of ice | kJ/mol | |
| accepted ΔH fusion per mole of ice | 6.01 | kJ/mol |
| % error |
Need some help solving this table. the answer I came up with seemed like it was way off. Can someone help?
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