More than 20 million tons of methanol, CH3OH, is produced annually, primarily via the following equilibrium reaction: Co(g) + 2 H2(g) – CH3OH(g) A,H° = -95 kJ mol-1 100 bar of gaseous CO and 100 bar of gaseous H2 are added to a sealed reaction apparatus at 250°C, and the system is allowed to reach dynamic equilibrium. Which of the following changes to the system will increase the yield of methanol? Select all that apply. OA piston inside the reaction apparatus is raised, increasing the volume of the gaseous mixture. OThe temperature is decreased to 200°C. O Methanol is removed by passing the gaseous mixture through a condenser. The total pressure inside of the reaction compartment is increased through the addition of 100 bar of argon gas. The temperature is increased to 300°C. An additional 100 bar of CO is added to the reaction apparatus. U Some H2 gas is removed. UA piston inside the reaction apparatus is compressed, reducing the volume of the gaseous mixture.
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.
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