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anonymous
 one year ago
At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and
oxygen:
2N
2
O
5
(g)
4NO
2
(g)
+
O
2
(g)
When the rate of formation of O
2
is 2.2
×
10

4
M/s, the rate of decomposition of N
2
O
5
is
__________ M/s.
anonymous
 one year ago
At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) When the rate of formation of O 2 is 2.2 × 10  4 M/s, the rate of decomposition of N 2 O 5 is __________ M/s.

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anonymous
 one year ago
Best ResponseYou've already chosen the best response.0please I need help with this worksheet

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0for each mole of O2 that is form in the reaction 2 moles of N2O5 has to be consumed then if you have the reaction produced 2.2 x 10^4 M/s of O2 you wil be able to figure out how much N2O5 has to be consumed by second to produce that amount of O2.

anonymous
 one year ago
Best ResponseYou've already chosen the best response.0\[Rate= \frac{ \Delta[N _{2}O _{5}] }{2 \Delta t}=\frac{ \Delta[O _{2}] }{ \Delta t}\] \[\frac{ \Delta[N _{2}O _{5}] }{\Delta t}=\frac{ 2\Delta[O _{2}] }{ \Delta t}\] \[{ \Delta[N _{2}O _{5}] }={ 2\Delta[O _{2}] }\]
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