English
Tamil Nadu Board of Secondary EducationHSC Science Class 11

What is the density of N2 gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K–1 mol–1)

Advertisements
Advertisements

Question

What is the density of N2 gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K–1 mol–1)

Options

  • 1.40 g/L

  • 2.81 g/L

  • 3.41 g/L

  • 0.29 g/L

MCQ
Advertisements

Solution

3.41 g/L

shaalaa.com
  Is there an error in this question or solution?
Chapter 6: Gaseous State - Evaluation [Page 181]

APPEARS IN

Samacheer Kalvi Chemistry - Volume 1 and 2 [English] Class 11 TN Board
Chapter 6 Gaseous State
Evaluation | Q I. 23. | Page 181

RELATED QUESTIONS

State and write the mathematical expression for Dalton’s law of partial pressure and explain it with a suitable example.


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.


The density of an ideal gas can be expressed as d = ____________.


If two moles of an ideal gas at 546 K occupy a volume of 44.8 L. What is the pressure of ideal gas at 546 K? (R = 0.0821 L atm mol-1 K-1)


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)


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.


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 After some oxygen is withdrawn from the cylinder, its gauge pressure drops to 11 atmospheric pressure at temperature 27°C. The mass of the oxygen withdrawn from the cylinder is nearly equal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]


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×