Calculate the number of grams of magnesium required to perform an experiment involving the reaction below to yield the following measurements: Mg (s) + 2 HCl (aq) → H2 (g) + MgCl2 (aq) The ideal gas equation is: PV = nRT The gas was collected over water. Initial Volume of Hydrogen Gas: 5.80 mL Final Volume of Hydrogen Gas: 39.45 mL Volume of Hydrogen Gas: ________ mL Temperature ˚C: 20.9 ˚ C Temperature K: ________ K Barometric Pressure 762.747 torr Vapor Pressure at 21.2 ˚C 18.536 torr Corrected Pressure ______________atm Experimental Gas Constant, R: 81.6 atm·mL/mol·K Moles of Hydrogen Gas: ___________moles of H2 Moles of Magnesium: ____________moles of Mg Mass of Magnesium: ___________grams of Mg
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.
Calculate the number of grams of magnesium required to perform an experiment involving the reaction below to yield the following measurements:
Mg (s) + 2 HCl (aq) → H2 (g) + MgCl2 (aq)
The ideal gas equation is: PV = nRT
The gas was collected over water.
Initial Volume of Hydrogen Gas: 5.80 mL
Final Volume of Hydrogen Gas: 39.45 mL
Volume of Hydrogen Gas: ________ mL
Temperature ˚C: 20.9 ˚ C
Temperature K: ________ K
Barometric Pressure 762.747 torr
Vapor Pressure at 21.2 ˚C 18.536 torr
Corrected Pressure ______________atm
Experimental Gas Constant, R: 81.6 atm·mL/mol·K
Moles of Hydrogen Gas: ___________moles of H2
Moles of Magnesium: ____________moles of Mg
Mass of Magnesium: ___________grams of Mg
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