Trichloroethylene, a widely used degreasing solvent for machine parts, is produced in a two-step reaction sequence. Ethylene is first chlorinated to yield tetrachloroethane, which is dehydrochlorinated to form trichloroethylene.

The standard heat of formation of liquid trichloroethylene is 276:2 kJ/mol.

(a) Use the given data and tabulated standard heats of formation of ethylene and hydrogen chloride to calculate the standard heat of formation of tetrachloroethane and the standard heat of the second reaction.

(b) Use Hess’s law to calculate the standard heat of the reaction

(c) If 300mol/h of C₂HCl₃(l) is produced in the reaction of Part (b) and the reactants and products are all at 25°C and 1 atm, how much heat is evolved or absorbed in the process? (Assume Q̇ = ΔḢ.)

(d) If the reaction of Part (c) were carried out and the final temperature in the reactor were 40°C instead of 25°C, how would it affect the problem solution? Explain your answer.

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C,H4(g) + 2C12(g) C,H,Cl4(1) + H2(g) AH; = -385.76 kJ C2H2CI4 (1) → C2HC13(1) + HCI(g)