Following question refer to one mole of chlorine gas.
(a) What is the volume occupied by this gas at STP?
(b) What will happen to volume of gas, if pressure is double?
(c) What volume will it occupy at $273^{\circ} C$ ?
(d) If the relative atomic mass of chlorine is 35.5, what will be the mass of 1 mole of chlorine gas?

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At N.T.P. the volume of a gas is found to be 273 ml. What will be the volume of this gas at 600 mm Hg and 273∘ C

The correct option is C 691.6 mlV2=P1V1T1(T2P2)=760600×546273×273=691.6ml

At N.T.P. the volume of a gas is found to be 273 ml. What will be the volume of this gas at 600 mm Hg and $273^{\circ}$ C

The correct option is C 691.6 ml
$V_{2} = \frac{P_{1} V_{1}}{T_{1}} (\frac{T_{2}}{P_{2}}) = \frac{760}{600} \times \frac{546}{273} \times 273 = 691.6 m l$