Chapter 5

The correct value of the gas constant \({ }^{\prime} R\) is close to (a) \(0.082\) litre-atmosphere \(\mathrm{K}\) (b) \(0.082\) litre-atmosphere \(\mathrm{K}^{-1} \mathrm{~mol}^{-1}\) (c) \(0.082\) litre-atmosphere \(^{-1} \mathrm{~K} \mathrm{~mol}^{-1}\) (d) \(0.082\) litre \(^{-1}\) atmosphere \(^{-1} \mathrm{~K} \mathrm{~mol}\).

Ideal gas equation is also called equation of states because (a) it depends on states of matter (b) it is a relation between four variables and describes the state of any gas (c) it is combination of various gas laws and any variable can be calculated (d) it is applicable to only ideal gases under STP conditions.

At what temperature \(28 \mathrm{~g}\) of \(\mathrm{N}_{2}\) will occupy a volume of 20 litres at 2 atm? (a) \(300.0 \mathrm{~K}\) (b) \(487.2 \mathrm{~K}\) (c) \(289.6 \mathrm{~K}\) (d) \(283.8 \mathrm{~K}\)

There is a standard value of temperature and pressure at which the molar volume of a gas is \(22.4 \mathrm{~L}\). The correct values are (a) \(273 \mathrm{~K}, 1 \mathrm{~atm}\) (b) \(300 \mathrm{~K}, 760 \mathrm{~mm}\) (c) \(25^{\circ} \mathrm{C}, 760 \mathrm{~mm}\) (d) \(373 \mathrm{~K}, 1 \mathrm{~atm}\)

How many number of moles of nitrogen will be present in \(2.24\) L of nitrogen gas at STP? (a) \(9.9\) (b) \(0.099\) (c) \(0.001\) (d) \(1.00\)

What volume in litres will be occupied by \(4.4 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) at STP? (a) \(22.4 \mathrm{~L}\) (b) \(44.8 \mathrm{~L}\) (c) \(12.2 \mathrm{~L}\) (d) \(2.24 \mathrm{~L}\)

Weight of \(\mathrm{CO}_{2}\) in a \(10 \mathrm{~L}\) cylinder at 5 atm and \(27^{\circ} \mathrm{C}\) is (a) \(200 \mathrm{~g}\) (b) \(224 \mathrm{~g}\) (c) \(44 \mathrm{~g}\) (d) \(89.3 \mathrm{~g}\)

The volume occupied by \(88 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) at \(30^{\circ} \mathrm{C}\) and 1 bar pressure will be \(\begin{array}{lll}\text { (a) } 5.05 \mathrm{~L} & \text { (b) } 49.8 \mathrm{~L}\end{array}\) (c) \(2 \mathrm{~L}\) (d) \(55 \mathrm{~L}\)

If 4 moles of an ideal gas at 300 K occupy volume of \(89.6 \mathrm{~L}\), then pressure of the gas will be (a) \(2 \mathrm{~atm}\) (b) \(1 \mathrm{~atm}\) (c) \(1.099 \mathrm{~atm}\) (d) \(2.910 \mathrm{~atm}\)

What will be the pressure of the gas mixture of \(3.2 \mathrm{~g}\) methane and \(4.4 \mathrm{~g}\) carbon dioxide contained in a \(9 \mathrm{dm}^{3}\) flask at \(27^{\circ} \mathrm{C}\) ? (a) \(0.82\) atm (b) \(8.314 \times 10^{4} \mathrm{~atm}\) (c) \(1 \mathrm{~atm}\) (d) \(1.8 \mathrm{~atm}\)