You visited us 1 times! Enjoying our articles? Unlock Full Access!

Electroplating

The decomposi...

Question

The decomposition of N2O5 in chloroform was followed by measuring the volume of O2 gas evolved: 2N2O5(CCl4) -------> 2N2O4(CCl4)+O2(g). The maximum volume of O2 gas obtained was 100cm^3. In 500 minutes ,90 cm^3 of O2 were evolved . The first order rate constant (in min^-1 ) for the disappearance of N2O5 is

Open in App

Solution

Suggest Corrections

Similar questions

N_{2} O_{5}

C C l_{4}

2 N_{2} O_{5} \to 4 N O_{2} + O_{2}

Time in minutes	10	15	20	25	$\infty$
The volume of $O_{2}$ evolved (in mL)	6.30	8.95	11.40	13.50	34.75

H_{2} O_{2}

I^{-}

t/min	3.0	6.0	9.0	$\infty$
Volume of $O_{2}$ evolved/ $c m^{3}$	6.2	11.8	16.8	60.6

H_{2} O_{2} (g) I^{-} - \to H_{2} O (l) + 1 / 2 O_{2} (g)

N_{2} O_{5}

30^{0} C

^{- 1}

O_{2}

=

O_{2}

=

N_{2} O_{5}

N_{2} O_{5} \to N_{2} O_{4} + 1 / 2 O_{2}

O_{2}

The decomposition of N₂O₅ is first order reaction and represented by

After 15 minutes the volume of O₂ produced is 9 cc and at the end of the reaction 35 cc. The rate constant is equal to

Join BYJU'S Learning Program