A) 4, 6
B) 5, 5
C) 2, 8
D) 8, 2
E) 6, 4
Correct Answer: E
Solution :
According to Daltons law, \[{{p}_{solute}}={{x}_{solute}}\times p\] where,\[{{p}_{solute}}=\]partial pressure of solute \[{{x}_{solute}}=\]fraction of solute p = total pressure Given, mass of \[{{N}_{2}}=56\text{ }g\] \[\therefore \]Moles of \[{{N}_{2}}({{n}_{{{N}_{2}}}})=\frac{56}{28}=2\,mol\] Mass of \[{{O}_{2}}=96g\] \[\therefore \] Moles of\[{{O}_{2}}({{n}_{{{O}_{2}}}})=\frac{96}{32}=3\,mol\] \[{{x}_{{{N}_{2}}}}=\frac{2}{2+3}=0.4\] \[{{x}_{{{O}_{2}}}}=\frac{3}{2+3}=0.6\] \[\therefore \] \[{{p}_{{{N}_{2}}}}={{x}_{{{N}_{2}}}}\times p=0.4\times 10=4\,atm\] \[{{p}_{{{O}_{2}}}}={{x}_{{{O}_{2}}}}\times p=0.6\times 10=6\,atm\]
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