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.
Advertisements
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?
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?
Solve the following.
Calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules
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
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.
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).
For an ideal gas, at constant temperature and pressure, the volume 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 is the density of water vapour at boiling point of water?
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)
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)
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?
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 ______.
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]
