The data below shows the change in concentration of dinitrogen pentoxide over time, at 330 K, according to the following process. 2N2O5(g) = 4NO2(g) + O2
[N2O5] Time (s)
0.100 0.00
0.066 200.00
0.044 400.00
a) Find the rate of disappearance of N2O5 from t=0 s to t=200s
b) Find the rate of appearance of NO2 from t=0 s to t =200s

A) Find the rate of disappearance of from t = 0 s to t = 200s

B) Find the rate of appearance of from t = 0 s to t = 200s

According to rate law,

For more information on rate of disappearance

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a)

b)

Explanation:

The reaction is :

Rate = Rate of disappearance of = Rate of appearance of

Rate =   =

Rate of disappearance of = =

a) Rate of disappearance of =

Rate of appearance of =

b) Rate of appearance of =  

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.