Advertisements
Advertisements
Question
Taking the volume of hydrogen as calculated in Q.19, what change must be made in Kelvin (absolute) temperature to return the volume to 2500 cm3 (pressure remaining constant)?
Advertisements
Solution
V1 = 714.29 cm3
P1 = P2 = P
T1 = 273 K
V2 = 2500 cm3
T2= ?
By using Charles's Law,
`("P"_1 "V"_1)/"T"_1 = ("PV"_2)/"T"_2`
Since P is constant, it cancels out.
`"V"_1/"T"_1 = "V"_2/"T"_2`
T2 = `("V"_2 xx "T"_1)/"V"_1`
T2 = `(2500 xx 273)/714.29`
T2 = 3.5 × 273
T2 = 955.5 K
∴ T2 = 3.5 times
∴ The temperature must be increased 3.5 times.
APPEARS IN
RELATED QUESTIONS
Give reasons for the following:
Mountaineers carry oxygen cylinders with them.
Choose the correct answer:
The volume-temperature relationship is given by
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.
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?
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.
Correct the following statement:
The volume of a fixed mass of a gas is directly proportional to its temperature, pressure remaining constant.
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?
According to Charles’s law, at constant pressure, the temperature is inversely proportional to volume.
