Advertisements
Advertisements
Question
If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct?
Options
Density is directly proportional to molar mass of the gas.
Greater the density greater is the molar mass of the gas.
If density, temperature and pressure is given ideal gas equation can be used to find molar mass.
All the above statements are correct.
Advertisements
Solution
All the above statements are correct.
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?
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.
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
At identical temperature and pressure, the rate of diffusion of hydrogen gas is `3sqrt3` times that of a hydrocarbon having molecular formula CnH2n–2. What is the value of n?
Equal moles of hydrogen and oxygen gases are placed in a container, with a pin-hole through which both can escape what fraction of oxygen escapes in the time required for one-half of the hydrogen to escape.
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?
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?
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.
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).
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 ____________.
Which of the following does not represent the ideal gas equation?
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?
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 ______.
