Advertisements
Advertisements
प्रश्न
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.
उत्तर
Given:
V = 0.5 m3,
P = 2.0 × 102 kPa = 2.0 × 105 Pa
T = 300 K,
R = 8.314 J K−1 m−1
To find: Number of molecules of methane gas
Formula: PV = nRT
Calculation: According to ideal gas equation,
n = `"PV"/"RT"`
`n =(2.0xx10^5xx0.5)/(8.314xx300)`
n = 40 mol
Number of molecules = n × NA = 40 × 6.022 × 1023 = 2.4088 × 1025 ≈ 2.409 × 1025
The number of molecules of methane gas present is 2.409 × 1025 molecules.
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?
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.
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?
Solve the following.
Calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
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
If the temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes
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?
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?
Why do astronauts have to wear protective suits when they are on the surface of the moon?
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.
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 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 ____________.
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)
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)
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.
