Question

2. Volume of vapour at STP calculations embeqxa 19s2o P-0905atm V, = 145.6 mL T = 90.0°0+273 . IS K V2-0-905)(45.6) 363.15 K 273 Te STP 213 K la de 363.IS o-987 P2o.987atm V2= /003.6ml /1 of c :lde =1.o03 L 3. Mass of vapour calculation Massot ratour= Mass of lask, caf and cemolensed liguid- Mass of flask and cat 92-754 8,-92.65%0g O.09 68 9 92.7586-92.6580 tob ot ajs:/1 =O./006gham 4. Calculate the volume that 1 mole of an ideal gas would occupy at STP (i.e. 0 °C and 100 kPa). 0.08206 Lath olk Pv- nRT nEImole V=MRT P T=0'C 1913 K PE l00 kPa -1atm l100md(o.0820 6 (23 ), RE 0. 082057 L atm mo! " k-l Lath V 216 Ve 22.4L /1 5, Molar mass of unknown calculation Molar mas= mass e Cendemsed vatour ampunt of cendlensed vapouwr V2 VSTPlImote .01 68 16 nSTP amole) /2

are these answers correct? how to do question 5

Answer 1

for question number 2, when I consider the value of STP temperature to 273.15 K and proceeding with the calculation gave a result of V2 = 100.417 ml. You are confused with placing the decimal point I guess. So please check it again.

question 4 is a standard one and yes your answer is right. I presume that Question 3 is right considering you have not provided the exact details of the process parameters.

As of question 5, First of all, you got the formula right

the total mass of vapor = No of moles X Molar mass of the vapor

now from the given data V2 = 100.417 ml form the question 2 and V(STP) = 22400 ml from question 4

hence no of moles = 100.417/22400 = 4.483 x 10^-3 moles

now Molar Mass = Wt of the vapor / No of moles = 0.0968 / (4.483 x 10^-3) = 21.5927 gms

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