What is the molar volume of an ideal gas at one atmospheric pressure and $273^{o} C$ temperature?

44.8 litre

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22.4 litre

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11.2 litre

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5.6 litre

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Solution

The correct option is D 44.8 litre
At 273 $K$ and 1 $a t m$ pressure, gas occupies 22.4 litres molar volume. In the given question, pressure $=$ 1 $a t m$ , $n$ = 1 $m o l$ and temperature $= 273^{o} C = 546 K$ . Thus, at 546 $K$ and 1 $a t m$ pressure, an ideal gas would occupy 44.8 litres of molar volume, as volume is directly proportional to temperature, at constant pressure. When the temperature doubles, the volume also doubles.

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Similar questions

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, 0 °C). Show that it is 22.4 litres.

Q. The volume of 10 moles of an ideal gas is 1 litre at 27

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and 1 atmospheric pressure. What is the volume (in litres) of 20 moles of same gas at same temperature and pressure?

State True or False.

At STP, the molar volume of an ideal gas is 22.4 litre.

Q. The molar volume of one mole of gas at one atmospheric pressure and

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Q. One mole of an ideal gas at standard temperature and pressure occupies 22.4 L(molar volume). What is the ratio of molar volume to the atomic volume of a mole of hydrogen ? (Take the size of hydrogen molecule to be about 1).

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What is the molar volume of an ideal gas at one atmospheric pressure and 273oC temperature?

What is the molar volume of an ideal gas at one atmospheric pressure and $273^{o} C$ temperature?