Advertisements
Advertisements
Question
What temperature would be necessary to double the volume of a gas initially at s.t.p. if the pressure is decreased by 50%?
Solution
P1 = 1 atm
P2 = `1 xx 50/100 = 1/2` atm
V1 = x cc
V2 = 2x cc
T1 = 273 K
T2 = ?
Using gas equation `("P"_1"V"_1)/"T"_1 = ("P"_2"V"_2)/"T"_2`
∴ T2 = `("P"_2"V"_2"T"_1)/("P"_1"V"_1)`
`"T"_2 = 1/2 xx (2"x" xx 273)/(1 xx "x") = 273` K
T1 = 273 - 273 = 0°C
RELATED QUESTIONS
What is the value of molar volume of a gas at STP?
Fill in the blank
Mass of 22.4 litre of a gas at STP is __________.
What volume of hydrogen sulphide at STP will burn in oxygen to yield 12.8g what volume of oxygen would be required for complete combustion?
If 112 cm3 of hydrogen sulphide is mixed with 120 cm3 of chlorine at STP, what is the mass of sulphur formed?
H2S + Cl2 → 2HCI + S
What volume of oxygen at STP is required to affect the combustion of 11 litres of ethylene [C2H4] at 273°C and 380 mm of Hg pressure?
\[\ce{C2H4 + 3O2 → 2CO2 + 2H2O}\]
When carbon dioxide is passed over red hot carbon, carbon monoxide is produced according to the equation :
\[\ce{CO2 + C -> 2CO}\]
What volume of carbon monoxide at S.T.P. can be obtained from 3 g of carbon?
800 cm3 of gas is collected at 650 mm pressure. At what pressure would the volume of the gas reduce by 40% of its original volume, the temperature remaining constant?
A sample of carbon dioxide occupies 30 cm3 at 15°C and 740 mm pressure. Find its volume at STP.
Water decomposes to O2 and H2 under suitable conditions as represented by the equation below:
\[\ce{2H2O -> 2H2 + O2}\]
The 2500 cm3 of H2 is subjected to `2 1/2` times increase in pressure (temp. remaining constant). What volume will H2 now occupy?
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.
