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A bubble of methane gas rises from the bottom of the North sea. What will happen to the size of the bubble as it rises to the surface? - Chemistry

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A bubble of methane gas rises from the bottom of the North sea. What will happen to the size of the bubble as it rises to the surface?

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उत्तर

According to Boyle’s law, the size of the bubble of methane gas increases as it rises to the surface.

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अध्याय 10: States of Matter - Exercises [पृष्ठ १५७]

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

संबंधित प्रश्न

Give reason for the following:

Gases exert pressure in all directions.


State the following:

The absolute temperature of a gas at 7°C


Convert the following temperature from degree Celcius to kelvin.

25° C


Convert the following temperature from degree Celcius to kelvin.

−197° C


Convert the following pressure value into Pascals.

107000 Nm−2


Convert −100° C to kelvin


Identify the gas laws from the following diagram.

Diagram Gas laws
______________

Identify the gas laws from the following diagram.

Diagram Gas laws
______________

Consider a sample of a gas in a cylinder with a movable piston.

Show diagrammatically the changes in the position of the piston, if pressure is increased from 1.0 bar to 2.0 bar at a constant temperature.


Consider a sample of a gas in a cylinder with a movable piston.

Show diagrammatically the changes in the position of the piston, if the temperature is decreased from 400 K to 300 K, and pressure is decreased from 4 bar to 3 bar.


Write the statement for Boyle’s law


Write the statement for Charles’ law


Solve the following.

The volume of a given mass of a gas at 0°C is 2 dm3. Calculate the new volume of the gas at constant pressure when the temperature is decreased by 10°C.


Solve the following.

At 0°C, a gas occupies 22.4 liters. How much hot must be the gas in celsius and in kelvin to reach a volume of 25.0 liters?


Use of hot air balloon in sports and meteorological observation is an application of


Assertion: Critical temperature of CO2 is 304 K, it can be liquefied above 304 K.

Reason: For a given mass of gas, volume is to directly proportional to pressure at constant temperature


State Boyle's law.


Explain the following observation.

Aerated water bottles are kept under water during summer


A sample of gas at 15°C at 1 atm. has a volume of 2.58 dm3. When the temperature is raised to 38°C at 1 atm does the volume of the gas Increase? If so, calculate the final volume.


A sample of gas has a volume of 8.5 dm3 at an unknown temperature. When the sample is submerged in ice water at 0°C, its volume gets reduced to 6.37 dm3. What is its initial temperature?


Volume of a balloon at 25°C and 1 bar pressure is 2.27 L. If the pressure of the gas in balloon is reduced to 0.227 bar, what is the rise in volume of a gas?


A certain mass of a gas occupies a volume of 2 dm3 at STP. At what temperature the volume of gas becomes double, keeping the pressure constant?


If 2 moles of an ideal gas at 546 K has volume of 44.8 L, then what will be it's pressure? (R = 0.082)


10 g of gas at one atomospheric pressure is cooled from 273.15°C to 0°C keeping the volume constant. What is the final pressure?


If 300 mL of a gas at 26.85°C is cooled to 6.85°C at constant pressure. What will be the final volume of gas?


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