Advertisements
Advertisements
प्रश्न
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
उत्तर
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
संबंधित प्रश्न
Give reasons for the following:
Mountaineers carry oxygen cylinders with them.
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?
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.
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?
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.
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.]
