हिंदी

If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct? - Chemistry

Advertisements
Advertisements

प्रश्न

If the density of a gas is measured at constant temperature and pressure then which of the following statement is correct?

विकल्प

  • 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.

MCQ
Advertisements

उत्तर

All the above statements are correct.

shaalaa.com
  क्या इस प्रश्न या उत्तर में कोई त्रुटि है?
अध्याय 10: States of Matter - Exercises [पृष्ठ १५७]

APPEARS IN

बालभारती Chemistry [English] Standard 11 Maharashtra State Board
अध्याय 10 States of Matter
Exercises | Q 2. (H) | पृष्ठ १५७

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?


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


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.


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.


The variation of volume V, with temperature T, keeping the pressure constant is called the coefficient of thermal expansion ie α = `1/"V"((∂"V")/(∂"T"))_"P"`. For an ideal gas α is equal to


What are ideal gases?


Give a suitable explanation for the following facts about gases.

Gases don’t settle at the bottom of a container


Would it be easier to drink water with a straw on the top of Mount Everest?


The unit of ideal gas constant (R) is ____________.


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?


What is the density of water vapour at boiling point of water?


At constant pressure, a quantity of an ideal gas occupies 1.0 × 10−2 dm3 volume at 200 K. At what temperature, the volume will be 2.0 × 10−3 dm3?


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 ____________.


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)


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.


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 ______.


The SI unit of pressure is:


Gay-Lussac's Law relates pressure and temperature at constant:


The ideal gas equation for n moles of gas is:


A hot air balloon rises because:


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×