Advertisements
Advertisements
Question
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
Advertisements
Solution
Given:
n = number of moles = 1 mol,
P = pressure = 101.35 kPa = 1.00025 atm ≈ 1 atm
T = Temperature = 20°C = 20 + 273.15 K = 293.15 K
R = 0.0821 dm3 atm K–1 mol–1
To find: Volume (V)
Formula: PV = nRT
Calculation:
According to ideal gas equation,
PV = nRT
∴ V = `("nRT")/"P"`
∴ V = `(1xx0.0821xx293.15)/1`
∴ V = 24.07 dm3
The volume of the given gas is 24.07 dm3.
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?
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.
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.
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.
When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules
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
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?
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).
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 ______.
The unit of ideal gas constant (R) is ____________.
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?
Which of the following graphs is not correct for 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.
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.
Gas equation, pV = nRT is obeyed by a gas in ______.
The graph of volume (V) versus absolute temperature (T) at constant pressure is ______.
Gay-Lussac's Law relates pressure and temperature at constant ______.
A pressure cooker works on the principle of ______.
A hot air balloon rises because ______.
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]
