Advertisements
Advertisements
प्रश्न
If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct?
पर्याय
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.
उत्तर
All the above statements are correct.
APPEARS IN
संबंधित प्रश्न
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?
Would it be easier to drink water with a straw on the top of Mount Everest or at the base? Explain.
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
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
The value of the gas constant R is
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?
What is the density of N2 gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K–1 mol–1)
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 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).
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?
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?
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)
If 10−4 dm3 of water is introduced into a 1 dm3 flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?
(Given: Vapour pressure of H2O at 300 K is 3170 Pa; R = 8.314 JK−1 mol−1)
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 ______.