Falling Behind in Studies? Join Our Performance Improvement Batch. Enroll For Free
One of our academic counsellors will contact you within 1 working day.
Click to Chat
1800-1023-196
+91-120-4616500
CART 0
Use Coupon: CART20 and get 20% off on all online Study Material
Welcome User
OR
LOGIN
Complete Your Registration (Step 2 of 2 )
What will be the pressure of the gas mixture when 0.5 l of h2 at 0.8 bar and 2 l of o2 at 0.7 bar are introduced in a 1 l vessel at 27℃?
Use gaseous formula , PV = nRT => n = PV/RTnow, 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/RTsimilarly for O2, pressure ( P ) = 0.7 bar , volume ( V ) = 2 Lmoles 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 Lnow, total pressure = 1.8/RT × RT/1 = 1.8 atm
Post Question
Dear , Preparing for entrance exams? Register yourself for the free demo class from askiitians.
points won -