Home
Class 11
PHYSICS
Estimate the total number of air molecul...

Estimate the total number of air molecules (inclusive of oxygen, nitrogen, water vapour and other constituents) in a room of capacity `25.0 m^(3)` at a tempreature of `27^(@) `C and 1 atm pressure.

Text Solution

Verified by Experts

The correct Answer is:
`6.117 xx 10^(26)`
`nN = PV //kT = 1.01 3 xx 10^(5) xx 25 //1.38 xx 10^(-23) xx 10^(-23) = 6.117 xx 10^(26) ( R = Nk)`
Promotional Banner

Topper's Solved these Questions

  • PROPERTIES OF MATTER

    ICSE|Exercise MODULE 3 (KINETIC THEORY OF GASES ) FROM KINETIC THEORY-rms SPEED , TEMPERATURE , PRESSURE|29 Videos

  • PROPERTIES OF MATTER

    ICSE|Exercise MODULE 4 ( TEMPERATURE ) CONCEPTUAL SHORT ANSWER QUESTIONS WITH ANSWERS|12 Videos

  • PROPERTIES OF MATTER

    ICSE|Exercise MODULE 3 (KINETIC THEORY OF GASES ) VERY SHORT ANSWER QUESTIONS|11 Videos

  • OSCILLATIONS

    ICSE|Exercise SELECTED PROBLEMS (OSCILLATION IN A TUNNEL BORED THROUGH THE EARTH)|2 Videos

  • SAMPLE QUESTION PAPER - 01

    ICSE|Exercise SECTION - D|12 Videos

Similar Questions

Explore conceptually related problems

Estimate the total number of air molecules (inclusive of oxygen, nitrogen, water vapour and other constituents) in a room of capacity 25.0 m^(3) at a temperature of 27^(@) C and 1 atm pressure. (Boltzmann constant = 1.38 xx 10^(-23) JK^(-1)) .

Total number of moles of oxygen atoms in 3 litre O_3 (g) at 27^@C and 8.21 atm are :

(a) What is meant by: (i) Colligative properties (ii)Molality of a solution (b) What concentration of nitrogen should be present in a glass of water at room temperature? Assume a temperature of 25^(@)C , a total pressure of 1 atmosphere and mole fraction of nitrogen in air of 0.678 . [ K_(H) for nitrogen =8.42xx10^(-7) M//mm Hg ]

Estimate the number of air molecules that are in a room 4.00 m by 6.00 m by 3.00 m at standard pressure and room temperature (293K).

The density of water is 1000kgm−3. The density of water vapour at 100∘C and 1 atmospheric pressure is 0.6kgm−3. The volume of a molecule multiplied by the total number gives what is called, molecular volume. Estimate the ratio (or fraction) of the molecular volume to the total volume occupied by the water vapour under the above conditions of temperature and pressure.

A flask contains 10^(-3)m^(3) gas. At a temperature, the number of molecules of oxygen at 3.0xx10^(22) . The mass of an oxygen molecule is 5.3xx10^(-26) kg and at that temperature the rms velocity of molecules is 400m/s. The pressure in N//m^(2) of the gas in the flask is ..............

The solubility of pure oxygen in water at 20 ^(@) C and one atmosphere pressure is 1.38 xx 10 ^(-3) mol L^(-1) Calculate the concentration of oxygen at 20 ^(@) C and partial pressure of 0.21 atm.

Total number of moles of oxygen atoms in 3 litre O_3 (g) at 27^@ C and 8.21 atm are : (a) 3 (b) 1 (c) 1 (d) None of these

At 760 torr pressure and 20^(@)C tempreature , 1 L of water dissolves 0.04 gm of pure oxygen or 0.02 gm of pure nitrogen. Assuming that dry air is compound of 20% oxygen and 80% nitrogen (by volume), the masses (in g/L) of oxygen and nitrogen dissolved by 1 L of water at 20^(@)C exposed to air at a total pressure of 760 torr are respectively :

If the number of molecules of SO_(2) (atomic weight=64) effusing through an orifice of unit area of cross-section in unit time at 0^(@)C and 1 atm pressure in n. the number of He molecules (atomic weight=4) effusin under similar conditions at 273^(@)C and 0.25 atm is: