$$1$$ mole of $$H2$$ gas is contained in a box of volume $$V=1.00$$ $$m3$$ at $$T1$$ $$=$$ $$300$$ K. The gas is heated to a temperature of $$T2$$ $$=$$ $$3000$$ K and the gas gets converted into a gas of hydrogen atoms. The final pressure would be (considering$$ all gases to be $$ideal)

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Infinity Learn · Accepted Answer

When the molecules break into atoms, the number of moles would become twice.Now, by ideal gas equationP $$=$$ Pressure of gas,n $$=$$ Number of molesR Gas constant,T TemperatureWe have $$pV=$$ nRTAs volume (V) of the container is constant.As gases break, number of moles becomes twice of initial number.so $$n2=2n1So$$ p∝nT⇒ $$p2p1=n2T2n1T1=2n1(3000)n1(300)=20$$⇒ $$p2=20p1Hence$$, final pressure of the gas would be $$20$$ times the pressure initially.

1 mole of H₂ gas is contained in a box of volume V=1.00 m³ at T₁ = 300 K. The gas is heated to a temperature of T₂ = 3000 K and the gas gets converted into a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

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1 mole of H2 gas is contained in a box of volume V=1.00 m3 at T1 = 300 K. The gas is heated to a temperature of T2 = 3000 K and the gas gets converted into a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

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1 mole of H₂ gas is contained in a box of volume V=1.00 m³ at T₁ = 300 K. The gas is heated to a temperature of T₂ = 3000 K and the gas gets converted into a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)