1.

Calculate Delta U reaction for the hydrogenation of acetalence at constant volume and at 77^(@)C. Given that -DeltaH_(f)(H_(2)O)= -678 kcal mole , Delta H_("comb")(C_(2)H_(2))= -310.1 kcal//ms^(2)

Answer»


Solution :Required equation is :
`C_(2)H_(2(G)) + H_(2(g)) rarr C_(2)H_(4(g)) ""DeltaH-DeltaU-=?`
`H_(2(g))+ (1)/(2)O_(2(g)) rarr H_(2)O(l) "" DeltaH- = -67.8 """…"`(1)
`C_(2)H_(2(g)) + (5)/(2)O_(2(g)) rarr 2CO_(2) + 2H_(2)O(l)"" DeltaH-=-310.1"""..."`(2)
`C_(2)H_(4) + 3O_(2(g)) rarr 2CO_(2(g)) + 2H_(2)O(l)"" DeltaH-=-337.2 """..."(3)`
`(1) + (2) -(3)`
`implies C_(2)H_(2(g)) rarr C_(2)H_(4(g))`
`DeltaH_(rxxn) = -67.8 - 310.1 + 337.2 = -40.7 KCal`
`DeltaH = DeltaU + Deltan(g)RT`
`-40.7= DeltaU +(-1) xx 2 10^(-3) xx 350`
`DeltaU= -40.7+.7`
`DeltaU=-40"KCal"//"mole"`


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