A) 427mm
B) 472mm
C) 319mm
D) 913mm
E) None of these
Correct Answer: A
Solution :
Ist case Volume \[{{V}_{1}}=250\,\,mL,\]\[{{V}_{2}}=1000\,\,mL\] Pressure \[{{p}_{1}}=720\,\,mm,\]\[{{p}_{2}}=?\,\,mm\] Applying Boyles law, \[1000\times {{p}_{2}}=720\times 250\] or \[{{p}_{2}}=\frac{720\times 250}{1000}=180\,mm\] Thus, the partial pressure due to nitrogen \[(p{{N}_{2}})=180\,mm.\]. IInd case \[{{V}_{1}}=380\,mL,\]\[{{V}_{2}}=1000\,mL\] \[{{p}_{1}}=650\,mm,\]\[{{p}_{2}}=?\,\,mm\] Applying Boyles law, \[1000\times {{p}_{2}}=380\times 650\] or \[{{p}_{2}}=\frac{380\times 650}{1000}=247\,mm\] Thus, the partial pressure due to oxygen \[({{p}_{{{O}_{2}}}})=247\,mm.\] If p is the final pressure of the gaseous mixture then according to Daltons Law of partial pressures, \[p={{p}_{{{N}_{2}}}}+{{p}_{{{O}_{2}}}}=180+247=427\,mm.\]
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