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प्रश्न
1 mole of H2 gas is contained in a box of volume V = 1.00 m3 at T = 300K. The gas is heated to a temperature of T = 3000K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal) ______.
विकल्प
same as the pressure initially.
2 times the pressure initially.
10 times the pressure initially.
20 times the pressure initially.
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उत्तर
1 mole of H2 gas is contained in a box of volume V = 1.00 m3 at T = 300K. The gas is heated to a temperature of T = 3000K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal) 20 times the pressure initially.
Explanation:
Consider the diagram, when the molecules break into atoms, the number of moles would become twice.
Now, by ideal gas equation
P = Pressure of gas
N = Number of moles
R = Gas constant
T = Temperature
PV = nRT
As the volume (V) of the container is constant.
As gases break the number of moles becomes twice of initial, so n2 = 2n1
So, P ∝ nT
⇒ `P_2/P_1 = (n_2T_2)/(n_1T_1) = ((2n_1)(3000))/(n_1 (300))` = 20
⇒ P2 = 20P1
Hence, the final pressure of the gas would be 20 times the pressure initially.
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