Advertisements
Advertisements
प्रश्न
Solve the following.
Calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
Advertisements
उत्तर
Given:
n = number of moles = 1.0 mol,
V = volume = 2.0 dm3
T = Temperature = 20.0°C = 20.0 + 273.15 K = 293.15 K
R = 0.0821 L atm K–1 mol–1
To find: Pressure (P)
Formula: PV = nRT
Calculation:
According to ideal gas equation,
PV = nRT
∴ P = `"nRT"/"V"`
∴ P = `(1.0xx0.0821xx293.15)/2.0`
∴ P = 12.03 atm
The pressure of the given helium gas is 12.03 atm.
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?
If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct?
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.
A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5g neon. If the pressure of the mixture of the gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture?
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
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
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.
What is the density of N2 gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K–1 mol–1)
What are ideal gases?
Why do astronauts have to wear protective suits when they are on the surface of the moon?
A combustible gas is stored in a metal tank at a pressure of 2.98 atm at 25°C. The tank can withstand a maximum pressure of 12 atm after which it will explode. The building in which the tank has been stored catches fire. Now predict whether the tank will blow up first or start melting? (Melting point of the metal = 1100 K).
A cold drink bottle contains 200 mL liquid, in which CO2 is 0.1 molar. Considering CO2 as an ideal gas the volume of the dissolved CO2 at S.T.P is ______.
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?
What is the density of water vapour at boiling point of water?
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)
An evacuated glass vessel weighs 40 g when empty, 135 g when filled with a liquid of density 0.95 g mL−1 and 40.5 g when filled with an ideal gas at 0.82 atm at 250 K. The molar mass of the gas in g mol−1 is ______.
(Given: R = 0.082 L atm K−1 mol−1)
100 g of an ideal gas is kept in a cylinder of 416 L volume at 27°C under 1.5 bar pressure. The molar mass of the gas is ______ g mol−1.
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 ______.
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 ______.
Gas equation, pV = nRT is obeyed by a gas in ______.
Gay-Lussac's Law relates pressure and temperature at constant ______.
The ideal gas equation for n moles of gas is ______.
A pressure cooker works on the principle of ______.
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 ______.
An oxygen cylinder of volume 30 litres has 18.20 moles of oxygen. After some oxygen is withdrawn from the cylinder, its gauge pressure drops to 11 atmospheric pressure at temperature 27°C. The mass of the oxygen withdrawn from the cylinder is nearly equal to:
[Given: R = `100/12`Jmol−1 K−1,and molecular mass of 12 O2 = 32, 1 atm pressure = 1.01 × 105 N/m]
