Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: charco on September 19, 2005, 02:39:50 AM
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can someone check please:
The first-order reaction:
2N2(g) ---> 2N2(g) + O2(g)
has a rate constant of 1.3 x 10-11 s-1 at 270°C and 4.5 x 10-10 s-1 at 350°C. What is the activation energy for this reaction?
(A) 15 kJ
(B) 30 kJ
(C) 68 kJ
(D) 120 kJ
I get a different answer using:
k = Ae^-(Ea/RT)
lnk = lnA – Ea/RT
ln(1.3 x 10-11) = lnA – Ea/(8.314 x 543)
and
ln(4.5 x 10-10) = lnA – Ea/(8.314 x 623)
subtract one from the other
ln(4.5 x 10-10) - ln(1.3 x 10-11) = – Ea/(8.314 x 623) + Ea/(8.314 x 543)
8.314[ln(4.5 x 10-10) - ln(1.3 x 10-11)] = Ea/543 - Ea/623
8.314[ln(4.5 x 10-10) - ln(1.3 x 10-11)] = (623Ea – 543Ea)/ (623 x 543)
8.314 x 623 x 543 [ln(4.5 x 10-10) - ln(1.3 x 10-11)] = 80Ea
2812534.7[-21.52 + 25.07] = 80Ea
(2812534.7 x 3.5449)/80 = Ea
Ea = 124806
Ea = 124.8kJ mol-1
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your working is correct.
in fact, the quantities quoted in your question are in 2 significant figures, so your final answer must be given in 2 significant figures, therefore your answer is correct.
Ea = 124.8kJ mol-1 = 120 kJ mol-1 (2s.f)
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Thanks geo - although I feel that it's somewhat inappropriate to not have it pointed out in the question!
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this is a MCQ. How much stuff do you think will be pointed out?