Question

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.

Answer 1

please I need help with this worksheet

Answer 2

for 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.

Answer 3

\[Rate= -\frac{ \Delta[N _{2}O _{5}] }{2 \Delta t}=\frac{ \Delta[O _{2}] }{ \Delta t}\]
\[-\frac{ \Delta[N _{2}O _{5}] }{\Delta t}=\frac{ 2\Delta[O _{2}] }{ \Delta t}\]
\[-{ \Delta[N _{2}O _{5}] }={ 2\Delta[O _{2}] }\]