Solutions_Manual_for_Organic_Chemistry_6th_Ed 70

Solutions_Manual_for_Organic_Chemistry_6th_Ed 70 - 4- 1 1...

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Unformatted text preview: 4- 1 1 (a) first order: the exponent of [ ( CH3h CCI ] i n the rate l aw = 1 ( b) zeroth order: [ CH30H ] d oes not appear in the rate law ( i ts exponent is zero) (c) first order: the sum of the exponents in the rate law = 1 + 0 = 1 4- 1 2 (a) first order: the exponent of [cyclohexene] i n the rate l aw = 1 ( b) second order: the exponent of [ B r2 ] in the rate law = 2 ( c) third order: the sum of the exponents in the rate law = 1 + 2 = 3 4- 1 3 (a) the reaction rate depends o n neither [ethylene] nor [hydrogen] , s o i t i s zeroth order in both species. The overall reaction must be zeroth order. (b) rate = kr (c) The rate law does not depend on the concentration of the reactants. It must depend, therefore, on the only other chemical present, the catal yst. Apparently, whatever is happening on the surface of the catalyst determines the rate, regardless of the concentrations of the two gases. Increasing the surface area of the catalyst, or simply adding more c atalyst, would accelerate the reaction . 4- 1 4 (a) t + 1 3 kJ/mole H CI + • CH3 ....................... �----- CH 4 + CI · (b) Ea = + 1 3 kJ/mole ( + 3 k cal/mole) (c) !ili0 = - 4 kJ/mole ( - 1 kcal/mole) 4- 1 5 (a) reaction coordinate _____ Cl 2 + • C H3 ./...... .......... . ....... .,. + i 4 k ca IImole t - 1 09 kJ/mole reaction coordinate (b) reverse: C H 3C I + C I · ( c) reverse: Ea = ----- ----• C l2 + CH 3 + 1 09 kJ/mole + + 4 kJ/mole = + 1 1 3 kJ/mole ( + 2 6 k callmole + + 1 k callmole = + 27 kcaVmole) 62 ...
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