Advertisements
Advertisements
प्रश्न
A fixed volume of a gas occupies 760cm3 at 27°C and 70 cm of Hg. What will be its vol. at s.t.p.
Advertisements
उत्तर
P1 = 70 CM OF Hg
V1 = 760 cm3
T1 = 27°C
P2 = 76 cm of Hg
V2 = ?
T2 = 273 K
Using the gas equation, `("P"_1"V"_1)/"T"_1 = ("P"_2"V"_2)/"T"_2`
`= (70 xx 760)/300 = (76 xx "V"_2)/273`
∴ V2 = `(70xx760xx273)/(300xx76) = 637`cm3
APPEARS IN
संबंधित प्रश्न
How did Charles's law lead to the concept of an absolute scale of temperature?
Choose the correct answer:
The absolute temperature value that corresponds to 27°C is
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.
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.
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?
The following question refers to one mole of chlorine gas.
What volume will it occupy at 273°C?
