Carbon disulfide can be prepared from coke (an impure form of carbon) and elemental sulfur. 4 C(s) + S3(s) → 4 CS,(1) AH° = +358.8 kJ Calculate the amount of heat absorbed when 1.66 mol S, is reacted at constant pressure. AH = kJ Calculate the amount of heat absorbed in the reaction of 179 g of carbon with excess sulfur. ΔΗ kJ Calculate the amount of CS, produced when 373 kJ of heat is absorbed. mass: g
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.
Thermochem homework.. thanks!
![**Preparation of Carbon Disulfide from Coke and Elemental Sulfur**
Carbon disulfide can be prepared from coke (an impure form of carbon) and elemental sulfur via the following chemical reaction:
\[
4 \text{C}(s) + \text{S}_8(s) \rightarrow 4 \text{CS}_2(l) \quad \Delta H^\circ = +358.8 \text{kJ}
\]
### Task 1: Calculate the amount of heat absorbed when 1.66 mol of \( \text{S}_8 \) is reacted at constant pressure.
\[
\Delta H = \underline{\phantom{00000000000}} \text{kJ}
\]
### Task 2: Calculate the amount of heat absorbed in the reaction of 179 g of carbon with excess sulfur.
\[
\Delta H = \underline{\phantom{00000000000}} \text{kJ}
\]
### Task 3: Calculate the amount of \( \text{CS}_2 \) produced when 373 kJ of heat is absorbed.
\[
\text{Mass:} \ \underline{\phantom{00000000000}} \text{g}
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