Aqueous hydrochloric acid reacts with solid calcium metal to form a solution of calcium chloride and hydrogen gas. The reaction is highly spontaneous and proceeds to completion. A chemist reacts 65.20 g calcium with excess hydrochloric acid at STP. You may assume the gas behaves ideally under all conditions. (a) What volume of hydrogen gas is produced over water? (b) What is the final concentration (in mol/L) of calcium chloride in the solution if the initial acid solution had a volume of 0.60 L? Assume no change in solution volume. (c) All of the hydrogen gas that evolved during the reaction is collected and held in a rigid flask with a volume of 11.30 L. If the pressure in the flask cannot exceed 3.85 atm, what is the maximum temperature at which the gas can be stored in the flask?
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.
Aqueous hydrochloric acid reacts with solid calcium metal to form a solution of calcium chloride and hydrogen gas. The reaction is highly spontaneous and proceeds to completion. A chemist reacts 65.20 g calcium with excess hydrochloric acid at STP. You may assume the gas behaves ideally under all conditions.
(a) What volume of hydrogen gas is produced over water?
(b) What is the final concentration (in mol/L) of calcium chloride in the solution if the initial acid solution had a volume of 0.60 L? Assume no change in solution volume.
(c) All of the hydrogen gas that evolved during the reaction is collected and held in a rigid flask with a volume of 11.30 L. If the pressure in the flask cannot exceed 3.85 atm, what is the maximum temperature at which the gas can be stored in the flask?
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