Advertisements
Advertisements
प्रश्न
800 cm3 of gas is collected at 654 mm pressure. At what pressure would the volume of the gas reduce by 40% of its original volume, the temperature remaining constant?
Advertisements
उत्तर
Given: V = 800 cm3
P = 654 mm
P1= ?
V1 = reduced volume = 40% of 800
= `(800 xx 40)/100`
= 320
Net V1 = 800 − 320
= 480 cm3
T = T1
Using the gas equation,
`(PV)/T = (P_1 V_1)/T_1`
`(800 xx 654)/T = (P_1 xx 480)/T_1`
Since T = T1
P1 = `(800 xx 654)/480`
= 1090 mm of Hg.
APPEARS IN
संबंधित प्रश्न
Copper sulphate solution reacts with sodium hydroxide solution to form a precipitate of copper hydroxide according to the equation :
2NaOH + CuSO4 → Na2SO4 + Cu (OH)2 ↓
(i) What mass of copper hydroxide is precipitated by using 200 gm of sodium hydroxide?
[H = 1, O = 16, Na = 23, S = 32, Cu = 64]
(ii) What is the colour of the precipitate formed?
Fill in the blank
Mass of 22.4 litre of a gas at STP is __________.
Solve the following:
The vapour density of a gas is 8. What would be the volume occupied by 24.0 of the gas at STP?
Oxygen oxidase ethyne to carbon dioxide and water as shown by the equation :
2C2H2 + 5O2 → 4CO2 + 2H2O
What volume of ethylene gas at STP is required to produce 8.4 dm3 of carbon dioxide at STP?
Calculate the mass and volume of oxygen at S.T.P., which will be evolved on electrolysis of 1 mole (18 g) of water.
The following question refers to one mole of chlorine gas.
What is the volume occupied by this gas at STP?
What volume of hydrogen and oxygen measured at S.T.P. will be required to prepare 1.8 g of water?
How much volume will be occupied by 2 g of dry oxygen at 27°C and 740 mm pressure?
A gas is to be filled from a tank of capacity 10,000 litres into cylinders each having capacity of 10 litres. The condition of the gas in the tank is as follows:
- The pressure inside the tank is 800 mm of Hg.
- The temperature inside the tank is −3°C.
When the cylinder is filled, the pressure gauge reads 400 mm of Hg and the temperature is 270 K. Find the number of cylinders required to fill the gas.
Water decomposes to O2 and H2 under suitable conditions, as represented by the equation below:
\[\ce{2H2O -> 2H2 + O2}\]
Taking the volume of H2 calculated in 5(b), what changes must be made in kelvin (absolute) temperature to return the volume to 2500 cm3 pressure remaining constant?
