The density of a gas at normal pressure and 0°C
temperature is 1.2 kg m Calculate : (i) the root-
mean-square velocity of the molecules of the gas at
0°C, (ii) the temperature at which the velocity will
become three times the initial velocity. (Normal
pressure = 1.0 x 109 Nm2).
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Given info : The density of a gas at normal pressure and 0°C temperature is 1.2 kg/m³
To find :
- the root mean square velocity of the molecule of the gas at 0°C.
- the temperature at which velocity becomes three times the initial velocity.
solution : root mean square velocity of the molecules is given by, v = √{3P/ρ}
P is atmospheric pressure i.e., 1.01 × 10⁵ N/m²
ρ is density of gas i.e., ρ = 1.2 kg/m³
so v = √{3 × 1.01 × 10⁵/1.2}
= 502.5 m/s
we know, root mean square velocity is also given by, v = √{3RT/M}
i.e., v ∝ √T
means, v₁/v₂ = √(T₁/T₂)
here 3v₁ = v₂ , T₁ = 0°C = 273 K
⇒v₁/3v₁ = √(273/T₂)
⇒9 × 273 = T₂
⇒T₂ = 2457 K
Therefore temperature of the gas would be 2457K.
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