https://media.pearsoncmg.com/bc/bc_0media_chem/chem_sim/calorimetry/Calor.php Use the link above to open up the Pearson Calorimetry Simulation. Follow the instructions below for your experiment: 1. Determine the final temperature of a mixture of 50 grams of water at 10 oC added to 120 grams of water at 80 oC. Use the simulator to check your answer. (Hint: This is a weighted average.)
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.
https://media.pearsoncmg.com/bc/bc_0media_chem/chem_sim/calorimetry/Calor.php
Use the link above to open up the Pearson Calorimetry Simulation. Follow the instructions below for your experiment:
1. Determine the final temperature of a mixture of 50 grams of water at 10 oC added to 120 grams of water at 80 oC. Use the simulator to check your answer. (Hint: This is a weighted average.)
2. Use the simulator to determine the temperature change of 80 grams of water initially at 20 oC (Note: When adding metals to water, the water temperature always starts at 20 oC, you do not need to set this parameter.) when a 15 gram piece of iron at 150 oC is placed in it. (To select iron, click on the “solids” tab and use the pop-up menu.)
3. Click the “show graph view” box and then click “replay” for the experiment in #2. Describe the resulting graph. How do the two lines on the graph compare? What is the main conclusion you can draw from the graph?
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