Question

Question 5.8 What will be the pressure of the gaseous mixture when 0.5 L of H2 at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1L vessel at 27°C?

Class XI States of Matter Page 153

Answer 1

use gaseous formula ,
PV = nRT => n = PV/RT
now,
moles of H2 = PV/RT
for H2, pressure ( P ) = 0.8 bar and volume ( V ) = 0.5 L ,
moles of H2 = 0.8 × 0.5/RT = 0.4/RT

similarly for O2,
pressure ( P ) = 0.7 bar , volume ( V ) = 2 L
moles of O2 = PV/RT
= 0.7 × 2/RT = 1.4/RT

hence, total number of moles = 0.4/RT + 1.4/RT
= 1.8/RT

now, Total pressure = n'RT/V' [ by gas formula]
here, n' is Total moles = 1.8/RT
V' is total volume = 1 L

now, total pressure = 1.8/RT × RT/1 = 1.8 atm

Answer 2

Answer:

I hope this is the correct answer .