A 0.825 mol sample of Ar(g) initially at 298 K and 1.00 atm Molar heat capacity at constant Type of gas (Crm) R R is held at constant volume while enough heat is applied to raise the temperature of the gas by 14.9 K. Assuming ideal gas behavior, calculate the amount of heat atoms linear molecules (q) in joules required to affect this temperature change and the total change in internal energy, AU. Note that some books use AE as the symbol for internal energy instead of nonlinear molecules 3R where R is the ideal gas constant Δυ. J AU = 155.17 J q =
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.
Specific heat capacity is the amount of heat that is required to rise a temperature of 1 kg substance by 10C.
The amount of heat is calculated by the formula,
Q = m C ∆T
Where,
Q represents heat
m represents mass
∆T represents difference in temperature
C represents specific heat capacity
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