Question 2 The important industrial chemical, vinyl chloride, can be made by the reaction between acetylene and hydrogen chloride: C2H2(g) + HCl(g) → CH2=CHCl(g) A suitable catalyst is mercury(II) chloride. The reaction produces substantial amounts of heat and the reaction vessel is water-cooled. a. Calculate ∆??R ° at 25 °C for the complete reaction of 1.00 mol of hydrogen chloride. b. Hence calculate ∆??R ° at 25 °C for the complete reaction of 1.00 kg of hydrogen chloride. c. Calculate the amount (in moles) and mass (in kg) of cooling water that would be needed to keep the reaction vessel at 25 °C, if the water were initially at 10 °C. d. Calculate the amount (in moles) and volume (in cubic metres) of C2H2 at a pressure of 200 kPa and a temperature of 25 °C that would be required to react with 1.00 kg of hydrogen chloride. You may assume C2H2 to be a perfect gas. Data: ∆?f (298 K) for C2H2 (g) = 226.73 kJ mol–1 ∆?f (298 K) for HCl(g) = –92.31 kJ mol–1 ∆?f(298 K) for CH2=CHCl(g) = 35.5 kJ mol–1 ?? for H2O(l) = 75.291 J K–1 mol–1
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.
Question 2
The important industrial chemical, vinyl chloride, can be made by the reaction between
acetylene and hydrogen chloride:
C2H2(g) + HCl(g) → CH2=CHCl(g)
A suitable catalyst is mercury(II) chloride. The reaction produces substantial amounts of heat
and the reaction vessel is water-cooled.
a. Calculate ∆??R
° at 25 °C for the complete reaction of 1.00 mol of hydrogen chloride.
b. Hence calculate ∆??R
° at 25 °C for the complete reaction of 1.00 kg of hydrogen chloride.
c. Calculate the amount (in moles) and mass (in kg) of cooling water that would be needed
to keep the reaction vessel at 25 °C, if the water were initially at 10 °C.
d. Calculate the amount (in moles) and volume (in cubic metres) of C2H2 at a pressure of
200 kPa and a temperature of 25 °C that would be required to react with 1.00 kg of
hydrogen chloride. You may assume C2H2 to be a perfect gas.
Data:
∆?f (298 K) for C2H2 (g) = 226.73 kJ mol–1
∆?f (298 K) for HCl(g) = –92.31 kJ mol–1
∆?f(298 K) for CH2=CHCl(g) = 35.5 kJ mol–1
?? for H2O(l) = 75.291 J K–1 mol–1
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