Hey there! We receieved your request
Stay Tuned as we are going to contact you within 1 Hour
One of our academic counsellors will contact you within 1 working day.
Click to Chat
1800-5470-145
+91 7353221155
Use Coupon: CART20 and get 20% off on all online Study Material
Complete Your Registration (Step 2 of 2 )
Sit and relax as our customer representative will contact you within 1 business day
OTP to be sent to Change
3.2 g of oxygen (At. weight = 16) and 0.2 g of hydrogen (At. wt. = 1) are placed in a 1.12 litre flask at 0°C. The total pressure of the gas mixture will be
(a) 1 atm
(b) 4 atm
(c) 3 atm
(d) 2 atm
choose and explain
There is a total of 0.2 moles of gas =>n=0.2
volume of container is 1.12L=>V=1.12L
temp. is 273 K=>T=273K
there fore by PV=nRT
pressure=4atm
there fore option 2 is correct
hope u like this
PLS APPROVE
You are dealing with diatomic oxygen ( molar mass 32g/mol ) and diatomic hydrogen ( 2g/mol ) Mol O2 in flask = 3.2/32 = 0.1 mol Mol H2 in flask = 0.2/2 = 0.1 mol H2 Total moles = 0.2mol Calculate pressure using gas equation: PV = nRT P * 1.12 = 0.2*0.082057*273 P = 4.480/1.12 P = 4.000 atm Pressure = 4atm - choice b) is correct.
Plz Approve!
Get your questions answered by the expert for free
You will get reply from our expert in sometime.
We will notify you when Our expert answers your question. To View your Question
Win Gift vouchers upto Rs 500/-
Register Yourself for a FREE Demo Class by Top IITians & Medical Experts Today !