Volume occupied by chlorine gas at $50^{o} C$ was $1.5$ litre. The pressure exerted was was $5$ atmosphere. If volume of vessel was kept constant then what will be the pressure at $80^{o} C$ ?

5.464

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4.28

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6.52

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7.42

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Solution

The correct option is A $5.464$
USing ideal gas equation
$P V = n R T$
At constant $V, n, P α T$
Thus $\frac{P}{T} = c o n s t a n t$
SO, $\frac{P_{1}}{T_{1}} = \frac{P_{2}}{T_{2}}$
Given $P_{1} = 5 a t m T_{1} = 323 K T_{2} = 353 K P_{2}$
$\frac{5 \times 353 K}{323 K} = P_{2} P_{2} = 5.464 a t m$

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