A fixed mass of a gas occupies a volume of 580 cm3 at a temperature of 17°C and a pressure of 750 mm. What volume will the gas occupy at that pressure and at a temperature of 47°C?
OR
Two gases of the same mass occupy at STP the volumes of 4480 mL and 5600 mL respectively. Find out the ratio of molar masses of the two gases.
V1 = 580 cm3 (initial volume)
T1 = 17°C = 17 + 273.15 = 290.15 K
T2 = 47°C = 47+273.15 = 320.15K
V2 = ? (final volume)
Charles’s Law: V_1\over T_1 = V_2\over T_2
⇒ V2 = V_1\over T_1 × T2
⇒ V2 = 580\over 290.15 × 320.15 = 638.16cm3
OR
Volume of Gas 1 (V1) = 4480 mL
Volume of Gas 2 (V2) = 5600 mL
For Gas 1: n1 = 4480/22400 = 0.2 moles
For Gas 2: n2 = 5600/22400 = 0.25 moles
From relation: M_1\over M_2 = n_2\over n_1
⇒ M_1\over M_2 = 0.25\over 0.2 = 5\over 4
The ratio of the molar masses of the two gases is 5:4.
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