Find the relative molecular mass of a gas, 0.546 g of which occupied 360 cm3 at 87oC and 380 mm Hg pressure. [1 litre of hydrogen at s.t.p. weights 0.09 g]
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Molar gas volume at STP = 22400cm³
v1= 360 cm³
p1=380mmHg
t1 = 87+273 = 360K
v2=?
p2 = 760mmHg
t2 = 273K
(p1v1)t1 = (p2v2)/t2
(380x360)/360 = (760xv2)/273
v2 = (380 x 273)/760
v2 = 136.5 cm³
If 136.5cm³ has a mass of 0.546g
∴ 22400cm³ = (22400x0.546)/136.5 = 89.6g
Note: 22400 is the volume of one mole of gas at STP
∴ Relative molecular mass of the gas = 89.6
v1= 360 cm³
p1=380mmHg
t1 = 87+273 = 360K
v2=?
p2 = 760mmHg
t2 = 273K
(p1v1)t1 = (p2v2)/t2
(380x360)/360 = (760xv2)/273
v2 = (380 x 273)/760
v2 = 136.5 cm³
If 136.5cm³ has a mass of 0.546g
∴ 22400cm³ = (22400x0.546)/136.5 = 89.6g
Note: 22400 is the volume of one mole of gas at STP
∴ Relative molecular mass of the gas = 89.6
Answered by
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Answer:89.5 amu
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