Advertisements
Advertisements
Question
The pressure on one mole of gas at s.t.p. is doubled and the temperature is raised to 546 K. What is the final volume of the gas ? [one mole of a gas occupies a volume of 22.4 litres at stp.]
Advertisements
Solution
One mole of gas occupies a volume of 22.4 lit. at s.t.p.
∴ V1 = 22.4 lit.
P1 = 1 atm.
T1 = 273 K
V2 = ?
P2 = 2 atm.
T2 = 546 K
Using gas equation `("P"_1"V"_1)/"T"_1 = ("P"_2"V"_2)/"T"_2`
V2 = `("P"_1"V"_1"T"_2)/("T"_1"P"_2)`
`= (1xx22.4xx546)/(273xx2)` = 22.4 lits.
APPEARS IN
RELATED QUESTIONS
Give the assumptions of the kinetic molecular theory.
State the law which is represented by the following graph:
State the following:
Ice point in absolute temperature
What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 temperature remaining constant?
Calculate the final volume of a gas 'X' if the original pressure of the gas at STP is doubled and its temperature is increased three times.
An LPG cylinder can withstand a pressure of 14.9 atmospheres. The pressure gauge of the cylinder indicates 12 atmospheres at 27°C. Because of a sudden fire in the building, the temperature rises. At what temperature will the cylinder explode?
A certain mass of gas occupied 850 ml at a pressure of 760 mm of Hg. On increasing the pressure it was found that the volume of the gas was 75% of its initial value. Assuming constant temperature, find the final pressure of the gas?
At a given temperature the pressure of a gas reduces to 75% of its initial value and the volume increases by 40% of its initial value. Find this temperature if the initial temperature was -10°C.
According to Charles’s law, at constant pressure, the temperature is inversely proportional to volume.
The following question refers to one mole of chlorine gas.
What volume will it occupy at 273°C?
