A calorimeter is a well insulated container that can be used to measure heat changes in a process. The heat capacity of a calorimeter can be determined by carrying out a process with a known amount of released heat. If the calorimeter is well insulated, we can assume that the heat lost to the surroundings is zero. We can calculate the heat capacity (C) of the calorimeter by measuring the change in heat qcal and the temperature change of the calorimeter. For an object like a calorimeter that is made up of more than one substance, we can use the following equation that relates the heat change of the calorimeter (qcal) to the heat capacity of the calorimeter (C) and the change in temperature (∆T). The relationship is q c a l = C × Δ T where the units of C are J ∘ C and the units of ∆T are ºC. If the calorimeter undergoes a heat change (qcal) of 475.85 and the temperature of the calorimeter goes from 29.19 ºC to 36.73 ºC, what is the C of the calorimeter in J?
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.
A calorimeter is a well insulated container that can be used to measure heat changes in a process. The heat capacity of a calorimeter can be determined by carrying out a process with a known amount of released heat. If the calorimeter is well insulated, we can assume that the heat lost to the surroundings is zero.
We can calculate the heat capacity (C) of the calorimeter by measuring the change in heat qcal and the temperature change of the calorimeter. For an object like a calorimeter that is made up of more than one substance, we can use the following equation that relates the heat change of the calorimeter (qcal) to the heat capacity of the calorimeter (C) and the change in temperature (∆T). The relationship is q c a l = C × Δ T where the units of C are J ∘ C and the units of ∆T are ºC.
If the calorimeter undergoes a heat change (qcal) of 475.85 and the temperature of the calorimeter goes from 29.19 ºC to 36.73 ºC, what is the C of the calorimeter in J?
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