Assuming ideal gas behaviour, the ratio of density of ammonia to that of hydrogen chloride at same temperature and pressure is: (Atomic wt. of $C l$ 35.5 u)

0.46

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1.46

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1.64

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0.64

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Solution

The correct option is A 0.46
We know the relation for ideal gas, $d = \frac{P M}{R T}$
Where, M is molar mass of gas
d is density of gas
P is pressure of the gas
R is universal gas constant
T is temperature

$(M)_{N H_{3}} = 17 u$
$(M)_{H C l} = 36.5 u$
$\frac{d_{N H_{3}}}{d_{H C l}} = \frac{(M)_{N H_{3}}}{(M)_{H C l}} = \frac{17}{36.5} = 0.46$

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Assuming ideal gas behaviour, the ratio of density of ammonia to that of hydrogen chloride at same temperature and pressure is: (Atomic wt. of Cl 35.5 u)

The correct option is A 0.46We know the relation for ideal gas, d=PMRT Where, M is molar mass of gas d is density of gas P is pressure of the gas R is universal gas constant T is temperature (M)NH3=17 u (M)HCl=36.5 u dNH3dHCl=(M)NH3(M)HCl=1736.5=0.46

Assuming ideal gas behaviour, the ratio of density of ammonia to that of hydrogen chloride at same temperature and pressure is: (Atomic wt. of $C l$ 35.5 u)