A) 16.4
B) 1.46
C) 0.64
D) 0.46
Correct Answer: D
Solution :
Ideal gas equation - \[PV=nRT\] \[n=m/M\] So,\[PV=mRT/M\] \[P=mRT/MV\] \[P=dRT/M\]s If temperature and pressure is constant then \[d\propto M\] \[{{d}_{1}}/{{d}_{2}}={{M}_{1}}/{{M}_{2}}\] (\[{{d}_{1}}\]and\[{{M}_{1}}\]are density and molecular mass of ammonia) (\[{{d}_{2}}\]and\[{{M}_{2}}\]are density and molecular mass of hydrogen chloride) \[{{d}_{1}}/{{d}_{2}}=17/36.5\] \[{{d}_{1}}/{{d}_{2}}=0.46.\] Note: P is pressure, V is volume, n is number of moles, R is ideal gas constant and T is absolute temperature. m is mass and M is molar mass. d is density.
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