You are collecting an ideal gas and need to determine the number of moles produced from a reaction. You start with 5.00 grams Calcium (s) and react it in water to collect the H2 (g) that is produced. Ca(s) + 2H2O(l) --> Ca(OH)2(aq) + H2(g) A. First determine the moles of Hydrogen gas that is produced if 100% of the 5.00 grams Calcium react with water. Note I have done the set-up for you in each selection below. I want you to use PV=nRT to determine the volume in Liters with
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.
You are collecting an ideal gas and need to determine the number of moles produced from a reaction. You start with 5.00 grams Calcium (s) and react it in water to collect the H2 (g) that is produced. Ca(s) + 2H2O(l) --> Ca(OH)2(aq) + H2(g)
A. First determine the moles of Hydrogen gas that is produced if 100% of the 5.00 grams Calcium react with water. Note I have done the set-up for you in each selection below. I want you to use PV=nRT to determine the volume in Liters with the conditions in this problem.
B. Determine the Volume of the hydrogen gas produced if collected at a temperature of 25.0\circ∘C and a pressure of 999 mmHg.
Check your units, R = 0.08206 \frac{\left(L\cdot atm\right)}{\left(mol\cdot K\right)}(mol⋅K)(L⋅atm)
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