Advertisements
Advertisements
प्रश्न
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
Advertisements
उत्तर
Given:
n = number of moles = 1 mol,
P = pressure = 101.35 kPa = 1.00025 atm ≈ 1 atm
T = Temperature = 20°C = 20 + 273.15 K = 293.15 K
R = 0.0821 dm3 atm K–1 mol–1
To find: Volume (V)
Formula: PV = nRT
Calculation:
According to ideal gas equation,
PV = nRT
∴ V = `("nRT")/"P"`
∴ V = `(1xx0.0821xx293.15)/1`
∴ V = 24.07 dm3
The volume of the given gas is 24.07 dm3.
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?
Answer in one sentence.
When a gas is heated the particles move more quickly. What is the change in the volume of a heated gas if the pressure is kept constant?
If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct?
State and write the mathematical expression for Dalton’s law of partial pressure and explain it with a suitable example.
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 pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
Consider the following statements
i) Atmospheric pressure is less at the top of a mountain than at sea level
ii) Gases are much more compressible than solids or liquids
iii) When the atmospheric pressure increases the height of the mercury column rises
Select the correct statement
Equal moles of hydrogen and oxygen gases are placed in a container, with a pin-hole through which both can escape what fraction of oxygen escapes in the time required for one-half of the hydrogen to escape.
Would it be easier to drink water with a straw on the top of Mount Everest?
A tank contains a mixture of 52.5 g of oxygen and 65.1 g of CO2 at 300 K the total pressure in the tanks is 9.21 atm. Calculate the partial pressure (in atm.) of each gas in the mixture.
The unit of ideal gas constant (R) is ____________.
At a constant pressure, an ideal gas has a volume of 200 cm3 at 25°C. If the gas is cooled to −3°C, what will be the final volume of a gas?
What mass of an oxygen gas will occupy 8.21 L of volume at 1 atm pressure and 400 K temperature?
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)
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?
A gas is heated from 273 K to 373 K at 1 atm pressure. If the initial volume of the gas is 10 L, its final volume would be ______.
The graph of volume (V) versus absolute temperature (T) at constant pressure is ______.
Gay-Lussac's Law relates pressure and temperature at constant ______.
The ideal gas equation for n moles of gas is ______.
The value of the universal gas constant R is ______.
A pressure cooker works on the principle of ______.
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 ______.
