Advertisements
Advertisements
Question
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
Solution
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
RELATED QUESTIONS
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.
Calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules
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
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?
Argon is an inert gas used in light bulbs to retard the vaporization of the tungsten filament. A certain light bulb containing argon at 1.2 atm and 18°C is heated to 85°C at constant volume. Calculate its final pressure in atm.
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?
The unit of ideal gas constant (R) 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?
At constant pressure, a quantity of an ideal gas occupies 1.0 × 10−2 dm3 volume at 200 K. At what temperature, the volume will be 2.0 × 10−3 dm3?
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)
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?
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 ______.
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:
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 ______.
