Advertisements
Advertisements
प्रश्न
State and write the mathematical expression for Dalton’s law of partial pressure and explain it with a suitable example.
Advertisements
उत्तर
Dalton’s law of partial pressure:
- Statement: The total pressure of a mixture of two or more non-reactive gases is the sum of the partial pressures of the individual gases in the mixture.
- Explanation:
Dalton’s law can be mathematically expressed as:
PTotal = P1 + P2 + P3 …(at constant T and V)
where, PTotal is the total pressure of the mixture and P1, P2, P3, … are the partial pressures of individual gases 1, 2, 3, … in the mixture.
For example, consider two non-reactive gases A and B. On mixing the two gases, the pressure exerted by individual gas A in the mixture of both the gases is called partial pressure of gas A (say P1). Likewise, the partial pressure of gas B is P2. According to Dalton’s law, the total pressure of the mixture of gas A and B at constant T and V will be given as:
PTotal = P1 + P2 - Schematic illustration of Dalton’s law of partial pressures:
APPEARS IN
संबंधित प्रश्न
Answer in one sentence.
The pressure that each individual gas would exert if it were alone in the container, what do we call it as?
Would it be easier to drink water with a straw on the top of Mount Everest or at the base? Explain.
Solve the following.
Nitrogen gas is filled in a container of volume 2.32 L at 32°C and 4.7 atm pressure. Calculate the number of moles of the gas.
Solve the following.
Calculate the number of molecules of methane in 0.50 m3 of the gas at a pressure of 2.0 × 102 kPa and a temperature of exactly 300 K.
When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules
A bottle of ammonia and a bottle of HCl connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be
If the temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes
The variation of volume V, with temperature T, keeping the pressure constant is called the coefficient of thermal expansion ie α = `1/"V"((∂"V")/(∂"T"))_"P"`. For an ideal gas α is equal to
Suggest why there is no hydrogen (H2) in our atmosphere. Why does the moon have no atmosphere?
Why do astronauts have to wear protective suits when they are on the surface of the moon?
For an ideal gas, at constant temperature and pressure, the volume is ____________.
What mass of an oxygen gas will occupy 8.21 L of volume at 1 atm pressure and 400 K temperature?
The density of an ideal gas can be expressed as d = ____________.
If two moles of an ideal gas at 546 K occupy a volume of 44.8 L. What is the pressure of ideal gas at 546 K? (R = 0.0821 L atm mol-1 K-1)
Which of the following does not represent the ideal gas equation?
A box contains 0.90 g of liquid water in equilibrium with water vapour at 27°C. The equilibrium vapour pressure of water at 27°C is 32.0 Torr. When the volume of the box is increased, some of the liquid water evaporates to maintain the equilibrium pressure. If the liquid water evaporates, then the volume of the box must be - litre (nearest integer) R = 0.0821 L atm K-1 mol-1.
(Ignore the volume of the liquid water and assume water vapours behave as an ideal gas)
Which of the following graphs is not correct for ideal gas?
A jar contains a gas and a few drops of water at T K. The pressure in the jar is 830 mm of Hg. The temperature of the jar is reduced by 1%. The vapour pressure of water at two temperatures are 30 and 25 mm of Hg. The new pressure in the jar is ______ mm of Hg.
If 10−4 dm3 of water is introduced into a 1 dm3 flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?
(Given: Vapour pressure of H2O at 300 K is 3170 Pa; R = 8.314 JK−1 mol−1)
In Duma's method, 0.52 g of an organic compound on combustion gave 68.6 mL N2 at 27°C and 756 mm pressure. What is the percentage of nitrogen in the compound?
120 g of an ideal gas of molecular weight 40 g mol−1 are confined to a volume of 20 L at 400 K.
Using R = 0.0821 L atm K−1 mol−1, the pressure of the gas is ______.
The SI unit of pressure is ______.
The value of the universal gas constant R is ______.
A hot air balloon rises because ______.
According to Boyle's Law, at constant temperature, the pressure of a gas is ______.
A tyre of a vehicle is filled with air having pressure 270 kPa at 27°C. The air pressure in the tyre when the temperature increases to 37°C is ______.
