Chemistry, 09.01.2020 01:31 chloedonyes
For the reaction, 2 n2o5--> 4 no2+o2, the rate of formation of no2 is 0.004 mol^-1 s^-1.a) calculate the rate of disappearance of n2o5.b) calculate the rate of appearance of o2.
Answers: 3
= ![-\frac{1d[N_2O_5]}{2dt}](/tpl/images/0447/6971/30fba.png)
= ![\frac{1d[NO_2]}{4dt}](/tpl/images/0447/6971/b576c.png)
= ![\frac{1d[O_2]}{dt}](/tpl/images/0447/6971/6b167.png)
![NO_2=+\frac{1d[NO_2]}{dt}=0.004mol^{-1}s^{-1}](/tpl/images/0447/6971/9cf34.png)
![N_2O_5=\frac{2}{4}\times \frac{1d[NO_2]}{dt}=\frac{2}{4}\times 0.004=0.002mol^{-1}s^{-1}](/tpl/images/0447/6971/202ca.png)
![\frac{1}{4}\times \frac{1d[NO_2]}{dt}=\frac{1}{4}\times 0.004=0.001mol^{-1}s^{-1}](/tpl/images/0447/6971/a8812.png)
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For the reaction, 2 n2o5--> 4 no2+o2, the rate of formation of no2 is 0.004 mol^-1 s^-1.a) calcu...
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