Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: serjio on February 14, 2020, 02:15:35 PM
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The frequency factor is 6.31 x 108 M s-1 and the activation energy is 10 kJ/mol for the gas phase reaction: NO(g)+ O3(g)->NO2(g)+O2(g). Calculate the rate constant for this reaction at 370 K.
I try to use k= A e ^Ea/RT but it always wrong. Can anyone help me about this :'( :'(
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can you show your work?
do you have consistent units?
do you have a set of choices to pick from for answers?
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I doubt about the "+" in the exponential.
You should develop an intuition for that. Learning formulas doesn't work, you must re-establish and double-check every time whether + or -, * or /, and so on.
The activation energy slows down the reaction. So could the "+" possibly be correct?
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enthalpy...
I usually write the arrhenius equation as
k = Ao * exp(-Ea / RT)
regardless, I was hoping that Serjio was going to respond and show us his math with how he handled (or missed) that +/- term. But he seems to have fled. Too bad.
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I doubt about the "+" in the exponential.
You should develop an intuition for that. Learning formulas doesn't work, you must re-establish and double-check every time whether + or -, * or /, and so on.uc browser (https://www.ucbrowser.vip/) shareit (https://shareit.onl/) appvn (https://appvn.onl/)
The activation energy slows down the reaction. So could the "+" possibly be correct?
agreed!!!
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Serjio...
you stated you tried to use the equation k = A * e^(Ea/RT) to calculate k but kept getting the wrong answer. I asked you to show your work. Where's the work?