1 mole of H 2 gas is contained in a box of volume V = 1.00 m 3 at T = 300 K . The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

Question

1 mole of H 2 ​ gas is contained in a box of volume V = 1.00 m 3 at T = 300 K . The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal), same as the pressure initially, 2 times the pressure initially, 10 times the pressure initially, 20 times the pressure initially

MARKS App · Accepted Answer

According to gas equation $ P V = n RT or \quad \frac{P_2 V_2}{T_2}=\frac{P_1 V_1}{T_1} \quad or \quad \frac{P_2}{P_1}=\frac{V_1}{V_2} \cdot \frac{T_2}{T_1} Here , T_2=3000 \mathrm{~K}, T_1=300 \mathrm{~K} S in ce \mathrm{H}_2 s pl i t s in t o h y d ro g e na t o m s , t h ere f ore v o l u m e b eco m e ha l f i . e . , V_2=\frac{1}{2} V_1 ​ ∴ P 1 ​ P 2 ​ ​ = 2 1 ​ V 1 ​ V 1 ​ ​ × 300 3000 ​ or P 1 ​ P 2 ​ ​ = 20 ​ $

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