Chemistry

2500 cm³ of hydrogen is taken at S.T.P. The pressure of this gas is further increased by two and and a half times (temperature remaining constant). What volume will hydrogen occupy now?

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V₁ = 2500 cm³

P₁ = 760 mm Hg

P₂ = increased by two and a half times

= (1 + $2\dfrac{1}{2}$ ) times of 760 mm Hg

= (1 + $\dfrac{5}{2}$ ) times of 760 mm Hg

= ( $\dfrac{7}{2}$ x 760) mm Hg

V₂ = ?

By Boyle's Law:

$\text{P}$

Substituting the values :

$760 \times 2500 = \dfrac{7}{2} \times 760 \times \text{V}$

∴ Final volume = $\dfrac{5000}{7}$ cm³

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