Question

ions? 6.114. Ozone reacts completely with NO, producing NO, and O. A 10.0 L vessel is filled with 0.280 mol of NO and 0.280 mol of O, at 350 K. Find the partial pressure of each product and the total pressure in the flask at the end of the reaction.

Answer 1

NO + O3   $\rightarrow$ NO2 + O2

Initial no.of moles 0.28 0.28 0 0

At the end of the reaction     0 0 0.28 0.28

Total number of moles of products, n  = 0.28 + 0.28 = 0.56

Temperature, T= 350 K

Volume of the flask, V = 10L

Universal gas constant, R = 0.0821 L.atm.K-1mole-1

As per ideal gas equation, PV = nRT

So, total pressure of the products$P=\frac{nRT}{V}=\frac{0.56\times 0.0821\times 350}{10}=1.61atm$

Molefraction of one component = No. of the moles of the component / Total no. of moles of all the components

Partial pressure of the gas = Molefraction of the gas x Total pressure

Total pressure of the products = 1.61 atm

Molefraction of NO2 = 0.28 / 0.56 = 0.5 Molefraction of O2 = 0.28 / 0.56 = 0.5

partial pressure of NO2 at the end of the reaction = 0.5 x 1.61 = 0.805 atm

partial pressure of O2 at the end of the reacion = 0.5 x 1.61 = 0.805 atm