Advertisements
Advertisements
प्रश्न
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.
Advertisements
उत्तर
Given:
V = 2.32 L,
P = 4.7 atm,
T = 32°C = 32 + 273.15 K = 305.15 K
R = 0.0821 L atm K−1 mol−1
To find: n = number of moles of gas
Formula: PV = nRT
Calculation:
According to the ideal gas equation,
PV = nRT
∴ n = `"PV"/"RT"`
∴ n = `(4.7xx2.32)/(0.0821xx305.15)`
∴ n = 0.435 moles
Number of moles of N2 gas in the given volume is 0.435 moles.
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.
At 25°C and 760 mm of Hg pressure, a gas occupies 600 mL volume. What will be its pressure at the height where the temperature is 10°C and the volume of the gas 640 mL?
Equal weights of methane and oxygen are mixed in an empty container at 298 K. The fraction of total pressure exerted by oxygen is
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
The value of the gas constant R is
At identical temperature and pressure, the rate of diffusion of hydrogen gas is `3sqrt3` times that of a hydrocarbon having molecular formula CnH2n–2. What is the value of n?
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)
Give a suitable explanation for the following facts about gases.
Gases don’t settle at the bottom of a container
Suggest why there is no hydrogen (H2) in our atmosphere. Why does the moon have no atmosphere?
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).
At constant temperature, a quantity of an ideal gas occupies 50 mL at 500 mmHg pressure. At what pressure, the volume will be 100 mL?
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?
The density of an ideal gas can be expressed as d = ____________.
At a constant pressure, the density of a certain amount of an ideal gas is ____________.
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.
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)
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)
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 SI unit of pressure is ______.
A pressure cooker works on the principle of ______.
According to Boyle's Law, at constant temperature, the pressure of a gas 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]
