If the percentage of nitrogen in an organic compound is 12.5% then the mass of organic compound taken so as to produce 50mL of N2 at 300K and 684mm Hg pressure is xg. The value of 503x is: (R=0.08atm-L/mol-K)
A
7.00
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B
7
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C
7.0
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Solution
Given; P=684mm Hg=684/760atm T=300K R=0.08atm-L/mol-K
Molecular mass of nitrogen =28g/mol
From, PV=nRT Weight of Nitrogen in organic compound=PV×M.wtRT =684×50×10−3×280.08×760×300=0.0525g % of N in organic comp. =Mass of N in organic compTotal mass of organic comp.(w)×100 ⇒12.5=0.0525w×100 ⇒w=0.42
So, 503x=7