English

Would it be easier to drink water with a straw on the top of Mount Everest or at the base? Explain. - Chemistry

Advertisements
Advertisements

Question

Would it be easier to drink water with a straw on the top of Mount Everest or at the base? Explain.

Short Note

Solution

When you drink through a straw, the pressure inside the straw reduces (as the air is withdrawn by mouth) and the liquid is pushed up to your mouth by atmospheric pressure. Thus, drinking with a straw makes use of pressure difference to force the liquid into your mouth. So, if the pressure difference is less it will be difficult to drink through a straw. On the top of Mount Everest, atmospheric pressure is very low. Hence, it will be difficult to drink water with a straw on the top of Mount Everest as compared to at the base.

shaalaa.com
Ideal Gas Equation
  Is there an error in this question or solution?
Chapter 10: States of Matter - Exercises [Page 158]

APPEARS IN

Balbharati Chemistry [English] 11 Standard
Chapter 10 States of Matter
Exercises | Q 3. (E) | Page 158

RELATED QUESTIONS

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?


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


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


Consider the following statements

i) Atmospheric pressure is less at the top of a mountain than at sea level

ii) Gases are much more compressible than solids or liquids

iii) When the atmospheric pressure increases the height of the mercury column rises

Select the correct statement


If the temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes


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


Suggest why there is no hydrogen (H2) in our atmosphere. Why does the moon have no atmosphere?


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.


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?


A cold drink bottle contains 200 mL liquid, in which CO2 is 0.1 molar. Considering CO2 as an ideal gas the volume of the dissolved CO2 at S.T.P 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?


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)


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 ______.


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×