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A gas cylinder is filled with 211 torr of N2 and 615 torr of F2 and...

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Chemistry

A gas cylinder is filled with 211 torr of N2 and 615 torr of F2and the resulting reaction forms NF3 at constant temperature andvolume. N2(g) + 3 F2(g) ⎯→ 2 NF3 (g). What is the total pressure,and what are the Mole Fractions of each gas, after the reaction?(Hint: think ICE) Total Pressure at the end of Rxn: _______________Mole Fraction of N2 = ___________ F2 = __________ NF3 =____________

Answer & Explanation Solved by verified expert
4.3 Ratings (705 Votes)
At constant T and V assuming ideal gas behavior PVnRT Pressure Pi is directly proportional to number ofmoles ni for each gasN2g 3 F2g 2 NF3 gAs per the stoichiometry of the reaction    See Answer
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