Rate of Reaction


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Vanessa Romero-Campos 2B
Posts: 39
Joined: Fri Sep 25, 2015 3:00 am

Rate of Reaction

Postby Vanessa Romero-Campos 2B » Sun Feb 25, 2018 11:42 pm

Can someone explain why -d[NO2]/dt=d[NO]/dt=2 d[O2]/dt
I'm confused about the 2 before the d[O2]/dt
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Jessica Patzlaff 1A
Posts: 28
Joined: Fri Sep 29, 2017 7:05 am

Re: Rate of Reaction

Postby Jessica Patzlaff 1A » Sun Feb 25, 2018 11:46 pm

In the chemical equation, the stoichiometric coefficients show that for every mol of O2 formed there are 2 mol of NO and NO2, so it O2 is forming half as fast. Thus, its rate would have to be doubled to equal the rate of NO being formed and NO2 being broken down.

Timothy Kim 1B
Posts: 62
Joined: Fri Sep 29, 2017 7:04 am

Re: Rate of Reaction

Postby Timothy Kim 1B » Sun Feb 25, 2018 11:46 pm

The 2 is there due to the ratio of the coefficients between the reactants and the products.

AnuPanneerselvam1H
Posts: 52
Joined: Fri Sep 29, 2017 7:07 am

Re: Rate of Reaction

Postby AnuPanneerselvam1H » Sun Feb 25, 2018 11:51 pm

Since the stoichiometric coefficients are 2 for NO2 and 1 for O2, the rate of O2 production will be half of that of NO2 depletion.

Kayla Tchorz-Dis 1F
Posts: 30
Joined: Thu Jul 13, 2017 3:00 am

Re: Rate of Reaction

Postby Kayla Tchorz-Dis 1F » Mon Feb 26, 2018 9:39 am

you just need to pay attention to the coefficients, and since o2 is half, theres half as much made


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