Advertisements
Advertisements
प्रश्न
Solve the following.
Calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0°C.
उत्तर
Given:
n = number of moles = 1.0 mol,
V = volume = 2.0 dm3
T = Temperature = 20.0°C = 20.0 + 273.15 K = 293.15 K
R = 0.0821 L atm K–1 mol–1
To find: Pressure (P)
Formula: PV = nRT
Calculation:
According to ideal gas equation,
PV = nRT
∴ P = `"nRT"/"V"`
∴ P = `(1.0xx0.0821xx293.15)/2.0`
∴ P = 12.03 atm
The pressure of the given helium gas is 12.03 atm.
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.
State and write the mathematical expression for Dalton’s law of partial pressure and explain it with a suitable example.
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.
A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5g neon. If the pressure of the mixture of the gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture?
Solve the following.
Calculate the volume of 1 mole of a gas at exactly 20°C at a pressure of 101.35 kPa.
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
Equal weights of methane and oxygen are mixed in an empty container at 298 K. The fraction of total pressure exerted by oxygen is
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?
Would it be easier to drink water with a straw on the top of Mount Everest?
Why do astronauts have to wear protective suits when they are on the surface of the moon?
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?
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 ____________.
The density of an ideal gas can be expressed as d = ____________.
Which of the following graphs is not correct for ideal gas?
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)
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.
