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Chemistry

Taking the volume of hydrogen as calculated in Q.16 what change must be made in Kelvin (absolute) temperature to return the volume to 2500 cm3 (pressure remaining constant).

Gas Laws

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Answer

V1 = Initial volume of the gas = 50007\dfrac{5000}{7} cm3
T1 = Initial temperature of the gas = 273 K

V2 = Final volume of the gas = 2500 cm3
T2 = Final temperature of the gas = ?

By Charles' Law:

V1T1=V2T2\dfrac{\text{V}1}{\text{T}1} = \dfrac{\text{V}2}{\text{T}2}

Substituting the values :

50007×273=2500T2T2=7×273×25005000T2=7×2732T2=3.5×273\dfrac{5000}{7 \times 273} = \dfrac{2500}{\text{T}2} \\[1em] \text{T}2 = \dfrac{7 \times 273 \times 2500}{5000} \\[1em] \text{T}2 = \dfrac{7 \times 273}{2} \\[1em] \text{T}2 = 3.5 \times 273 \\[1em]

∴ Final temperature = 3.5 times of Kelvin temperature.

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