Calculate:

(a) the gram molecular mass of chlorine if $308 c m^{3}$ of it at STP weiths, 0.979 g,
(b) the volume of 4 g of $H_{2}$ at 4 atmosphere,
(c) the mass fo oxygen in 2.2 litres of $C O_{2}$ at STP.

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Solution

(a).

Find the gram molar mass of the Chlorine gas

$G r a m M o l a r m a s s o f t h e C l_{2} g a s = \frac{D e n s i t y \times R \times T e m p e r a t u r e}{P r e s s u r e}$
At STP,
Temperature = $0^{\circ} C + 273 K = 273 K$

Pressure = $1 a t m$

Volume = $308 m l = 0.308 L$

Density = $\frac{m a s s}{v o l u m e}$ = $\frac{0.979 g}{0.308 L} = 3.1785 g / L$

$G r a m M o l a r m a s s o f t h e C l_{2} g a s = \frac{3.1785 g / L \times 0.0821 a t m L / m o l K \times 273 K}{1 a t m} = 71.24 g / m o l$

(b). Assuming the temperature to be 273k
PV=nRT
thus V= $\frac{n R T}{P}$
n=no.of moles= $\frac{4 g r a m s}{2 g / m o l} = 2 m o l e s o f H_{2}$
Thus V = $\frac{2 m o l e s \times 0.0821 a t m L / m o l K \times 273 K}{4 a t m} = 11.2 L i t e r s o f H_{2}$

(c) The mass of oxygen in 2.2 liters of $C O_{2}$ at STP.

At STP condition, 1 mol = 22.4 Liters.

Moles of $C O_{2}$ = $\frac{2.2 L}{22.4 L / m o l} = 0.098 m o l e s o f C O_{2}$

Mass of $C O_{2}$ = $0.098 m o l e s o f C O_{2} \times 44.01 g / m o l = 4.322 g r a m s C O_{2}$

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Similar questions

Calculate:

a) the gram molecular mass of chlorine if 308 cm cube of it at STP weighs 0.979 grams

B) the volume of 4 gram of H2 at 4 atmospheres.

C) the mass of oxygen in 2.2 litres of carbon dioxide at STP

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Calculate: (a) the gram molecular mass of chlorine if 308cm3 of it at STP weiths, 0.979 g, (b) the volume of 4 g ofH2 at 4 atmosphere, (c) the mass fo oxygen in 2.2 litres of CO2 at STP.

Calculate:

(a) the gram molecular mass of chlorine if $308 c m^{3}$ of it at STP weiths, 0.979 g,
(b) the volume of 4 g of $H_{2}$ at 4 atmosphere,
(c) the mass fo oxygen in 2.2 litres of $C O_{2}$ at STP.