Advertisements
Advertisements
Question
2500 cm3 of hydrogen is taken at STP. The pressure of this gas is further increased by two and a half times (temperature remaining constant). What volume will hydrogen occupy now?
Advertisements
Solution
V1 = 2500 cm3
P1 = 1 atm = 760 mm
T1 = 273 K
V2= ?
T2 = 273 K
`"P"_2 = 760 xx 5/2 + 760 = 1900 + 760 = 2660 "mm"`
`("P"_1 "V"_1)/"T"_1 = ("P"_2 "V"_2)/"T"_2`
`(760xx2500)/273 = (2660xx"V"_2)/273`
`"V"_2 = 5000/7 = 714.29 "cm"^3`
APPEARS IN
RELATED QUESTIONS
State the following:
Ice point in absolute temperature
88 cm3 of nitrogen is at a pressure of 770 mm mercury. If the pressure is raised to 880 mmHg, find by how much the volume will diminish, the temperature remaining constant.
It is found that on heating a gas its volume increases by 50% and its pressure decreases to 60% of its original value. If the original temperature was −15°C, find the temperature to which it was heated.
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?
State Charles's law.
Give its
(i) graphical representation,
(ii) mathematical expression
(iii) significance
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?
Fill in the blank with the correct word, from the words in option:
If the temperature of a fixed mass of a gas is kept constant and the pressure is increased, the volume correspondingly _______.
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.]
The following question refers to one mole of chlorine gas.
What volume will it occupy at 273°C?
