Advertisements
Advertisements
प्रश्न
A given amount of gas A is confined in a chamber of constant volume. When the chamber is immersed in a bath of melting ice, the pressure of the gas is 100 cmHg.
- What is the temperature when the pressure is 10cmHg?
- What will be the pressure when the chamber is brought to 100°C
Advertisements
उत्तर
(a) V1 = V2 = V
P1 = 100 cm Hg
T1 = 273 K
P2 = 10 cm Hg
T2= ?
`("P"_1 "V"_1)/"T"_1 = ("P"_2 "V"_2)/"T"_2`
`(100 xx"V")/273 = (10 xx"V")/"T"_2`
`"T"_2 = 27.3 "K"`
(b) V1 = V2 = V
P1 = 100 cmHg
P2= ?
T1 = 273 K
T2 = 373 K
`("P"_1 "V"_1)/"T"_1 = ("P"_2 "V"_2)/"T"_2`
`(100 xx"V")/273 = ("P"_2 xx"V")/373`
`"P"_2 = 136.63 "cm of Hg"`
APPEARS IN
संबंधित प्रश्न
If 6 liters of hydrogen and 4 liters of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas.
The equations given below relate to the manufacture of sodium carbonate (Molecular weight of Na2CO3 = 106).
- \[\ce{NaCl + NH3 + CO2 + H2O -> NaHCO3 + NH4Cl}\]
- \[\ce{2NaHCO3 -> Na2CO3 + H2O + CO2}\]
Equations (1) and (2) are based on the production of 21.2 g of sodium carbonate.
- What mass of sodium hydrogen carbonate must be heated to give 21.2 g of sodium carbonate?
- To produce the mass of sodium hydrogen carbonate calculated in (a), what volume of carbon dioxide, measured at STP, would be required?
A gas cylinder contains 24 × 1024 molecules of nitrogen gas. If Avogadro's number is 6 × 1023 and the relative atomic mass of nitrogen is 14, calculate the volume of nitrogen at STP in dm3.
What is the mass of 56 cm3 of carbon monoxide at STP?
(C = 12 ,O = 16)
How much volume will be occupied by 2 g of dry oxygen at 27°C and 740 mm pressure?
From the equation:
\[\ce{C + 2H2SO4 -> CO2 + 2H2O + 2SO2}\]
Calculate the volume of sulphur dioxide measured at STP, liberated at the same time.
Hydrogen sulphide gas burns in oxygen to yield 12.8 g of sulphur dioxide gas as under:
\[\ce{2H2S + 3O2 -> 2H2O + 2SO2}\]
Calculate the volume of hydrogen sulphide at STP. Also, calculate the volume of oxygen required at STP which will complete the combustion of hydrogen sulphide determined in litres.
Write the values of:
standard pressure in:
(i) atm
(ii) mm Hg
(iii) cm Hg
(iv) torr
What temperature would be necessary to double the volume of a gas initially at s.t.p. if the pressure is decreased by 50%?
Which of the following would occupy 22.4 litres at S.T.P.?
- 32 g of oxygen gas
- 2 moles of hydrogen gas
- 6.022 × 1023 molecules of ammonia
[Atomic weights: O = 16, H = 1, N = 14]
