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)

(a) Same as the pressure initially

(b) 2 times the pressure initially

(c) 10 times the pressure initially

(d) 20 times the pressure initially

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Payal Gupta | Contributor-Level 10

8 months ago

This is a multiple choice answer as classified in NCERT Exemplar

(d) When number of molecules breaks then number of moles would become double.

P $\propto n T$ where n is the number of moles and T is temperature of ideal gas

As gases breaks number of moles becomes twcice of initial so n₂ =2n₁

$\frac{P_{2}}{P_{1}} = \frac{n_{2} T_{2}}{n_{1} T_{1}} = \frac{2 n_{1} (3000)}{n_{1} (300)}$ = 20

p₂=20p₁

so 20 tim

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physics ncert solutions class 11th 2023

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