Solid phosphorus (P) and chlorine (C1₂) gas react to form solid phosphorus pentachloride (PC15). Suppose you have 11.0 mol of P and 7.0 mol of Cl₂ in a reactor. Could half the P react? If you answered yes, calculate how many moles of PC15 would be produced after half the P was used up. Round your answer to the nearest 0.1 mol. Oyes O no mol X
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.
Given that,
Solid phosphorus (P) and chlorine (Cl2) gas react to form solid phosphorus pentachloride (PCl5)
If 11.0 mol of P and 7.0 mol of Cl2 reacted we need to find whether half of the P can react or not
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