1.

Consider the decomposition of N_2O_(5(g)) to form NO_(2(g)) and O_(2(g)) . At a particular instant N_2O_5 disappears at a rate of 2.5xx10^(-2) "mol dm"^(-3)s^(-1) . At what rates are NO_2 and O_2 formed ? What is the rate of the reaction ?

Answer»

Solution :`2N_2O_5(g)rarr4NO_(2(g))+O_2(g))`
from the stoichiometry of the REACTION of the reaction.
`-1/2(d[N_2O_5])/(dt)=1/4(d[NO_2])/(dt)=-(d[NO_2])/(dt)=2(-d[N_2O_5])/(dt)`
RATE of disappearance of `N_2O_(5(g))` is `2.5xx10^(-2) "mol dm"^(-3)s^(-1)`
`:.` The rate of formation of `NO_2` at this TEMPERATURE is `2xx2.5xx10^(-2)=5xx10^(-2)"mol dm"^(3)s^(-1)` .
`-1/2(d[N_2O_5])/(dt)=-(d[O_2])/(dt)`
`:. (d[O_2])/(dt) = 1/2xx2.5xx10^(-2) "mol dm "^(-3)s^(-1)=1.25xx10^(-2)" mol dm "^(-3)s^(-1)`


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