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Question

In an evacuated closed isolated chamber at 250oC. .02 mole PCl5 and .01 mole Cl2 are mixed (PCl5PCl3+Cl2). At equilibrium density of mixture was 2.49g/L and pressure was 1 atm. The number of total moles at equilibrium will be approximately:

A
0.012
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B
0.022
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C
0.032
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D
0.046
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Solution

The correct option is D 0.046
PV=mMRT
PM=dRT
Mmix=dmixRTP=2.49×0.0821×5231=106.91g
Mmix=xPCl5MPCl5+xCl2MCl2+xPCl3MCl3
PCl5PCl3+Cl2
0.02αα+0.01+α
Total moles=0.02α+α+0.01+α=0.03+α
106.91=(0.02α)208.50.03+α+(0.01+α)710.03+α+α×137.50.03+α
Solving this, we get α=0.0157
Total moles=0.03+0.0157=0.0457=0.046moles

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