56.00cm³ of a gas at S.T.P. weighed 0.11g. What is the vapour density of the gas?
[Molar volume of a gas at S.T.P = 22.4dm³]

mralz

12 years ago

Molar Volume of the gas 22.4dm3 to cm3= 22.4 * 1000= 22400cm3, so molar mass in gram 0.11 * molar volume (0.11g * 22,400=2,464 ÷ by 56.00cm3 which will give 44.00. We can't stop here since we where told to calculate Vapour density so vapour density from its derived formula = 1/2 * 44.00 which will give= 22.00

VictorAustin

10 years ago

We can also put it dis way.1000cm3 of hydrogen at s.t.p weighs 0.11g. :-56.00cm3 of hydrogen will weigh 56.00/1000*0.09g=0.005.bt vapour density=mass of a givn vol of gas/mass of equal vol of hydrogen.therefore we have vapour density of d gas to b mass of 56cm3 of d gas/mass of 56cm3 of hydrogen=0.11/0.005=22.d 0.09g/mol is d density of hydrogen @ s.t.p.

Anela

1 year ago

vol given=56cm³
mass = 0.11
Vol at STP = 22.4dm³( convert to cm³ to suit the question)= 22.4×1000= 22400

if; 56cm³ = 0.11
22400cm³= x
CROSS MULTIPLY ✖️

56x=0.11×22400
56x=2464
x=2464÷56
= 44


RECALL;
V.D=MM/2
= 44/2
22(ANS)

jamesblacq

8 years ago

wow bt am till confuse abt hw 44 was divided by 2

olucube111

11 years ago

perfectly correct