Advertisements
Advertisements
Question
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?
Solution
P = 14.9 atm
V = 28 cm3
T = ?
P1 = 12 atm
V = V1
T1 = 300 K
Using gas equation,
`("P" "V")/"T" = ("P"_1 "V"_1)/"T"_1`
`(14.9xx"V")/"T" = (12xx"V")/300`
T = 372.5 K
T = 372.5 - 273 = 99.5 °C
APPEARS IN
RELATED QUESTIONS
Explain Charles's law on the basis of the kinetic theory of matter.
State the following:
Ice point in absolute temperature
2 liters of gas is enclosed in a vessel at a pressure of 760 mmHg. If the temperature remains constant, calculate pressure when volume changes to 4 dm3.
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.
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?
Give its
(i) graphical representation,
(ii) mathematical expression
(iii) significance
Correct the following statement:
The volume of a fixed mass of a gas is directly proportional to its temperature, pressure remaining constant.
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?
