Question

not from Google please

​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​

Answer 1

Answer:

22.4 liters

Explanation:

⇒We know that the ideal gas equation: PV = nRT

⇒Where, R is the universal gas constant = 8.314 J mol-1 K-1

⇒n = Number of moles = 1

⇒T = Standard temperature = 273 K

⇒P = Standard pressure = 1 atm = 1.013 × 105 Nm-2

∴Thus,  V = (nRT)/p

= (1 x 8.314 x 273)/( 1.013 × 105)

= 0.0224 m3

= 22.4 liters

∴Thus, it is proved that the molar volume of a gas at standard temperature and pressure is 22.4 liters.

Answer 2

Required solution :-

To Prove,

The molar volume of a gas at standard temperature and pressure is 22.4 liters.

We know that,

• n = Number of moles
• r = Universal gas constant
• t = Standard temperature
• p = Standard pressure

By the equation,

$\underline{\boxed{\sf V=\dfrac{nRT}{P} }}$

Given that,

Universal gas constant (r) = 8.314 J mol⁻¹ K⁻¹

Number of moles (n) = 1

Standard temperature (t) = 273 K

Standard pressure = 1 atm (p) = 1.013 × 10⁵ Nm⁻²

Substituting their values,

$\sf =\dfrac{1 \times 8.314 \times 273}{1.013 \times 10^5}$

$\sf =0.0224 \ m^3$

$\sf = 22.4 \ litres$

Therefore, it is proved that the molar volume of a gas at standard temperature and pressure is 22.4 litres.