Question

Calculate the volume of 4 70cm3 of
gas at 27°C, whould occupy at 22 C
åt constant pressure?​

Answer 1

Answer:

6.23L

Explanation:

Given wCO=7g,P=(750/760)atm

mCO=28,T=300K

PV=(w/m)RT

∴750760×V=728×0.0821×300

or V=6.23litre .

Answer 2

Solution:

As per the given data,

• V₁ = 470 cm³ = 0.470 L (dm³)

In order to convert cm³ into dm³(L) divide by 1000

• T₁ = 273 + 27 = 300 K
• T₂ = 273 + 22 = 295 K

As per the ideal gas equation,

$\dag \: \boxed{\sf{PV = nRT }}$

here,

• P = pressure
• V = volume
• n = moles
• R = universal gas constant
• T = temperature

On rearranging,

⇒ V/T = nR/P

All the terms on the R.H.S are constant.

⇒ V/T = constant

From this, we can conclude that,

• V ∝ T

Charles Law

This law states that the volume of an ideal gas is directly proportional to its temperature at constant pressure.

Hence,

⇒ V₁ / T₁ = V₂ / T₂

⇒ V₂ = V₁ x T₁ / T₂

Now let's substitute the values,

⇒ V₂ = 0.470 x 300/295

⇒ V₂ = 141 / 295

⇒ V₂ = 0.477 L (dm³)