Two flasks, each 4.0 L, are connected to each
other. One flask contains O2 at 15 atm. The
other flask contains N2 at 7.0 atm. The gases
are allowed to mix. What is the mole fraction
of O2?
1. 0.26
2. Cannot be determined
3. 0.75
4. 0.93
5. 0.32
6. 0.68
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Verified answer
(15) / (15 + 7) = 0.68
So answer 6.
Moles gas A = pv/rt = 1.5atm x 2L / (zero.0821L-atm/mole-okay x 298K) = zero.123moles fuel A moles fuel B = 0.35atm x 2.5L / (zero.0821L-atm/mole-okay x 298K) = 0.036moles gas B 0.123moles A requires 2.5x moles of B or zero.308moles B, B = limiting reactant 0.036moles B x (2A / 5B) = zero.0144moles A consumed leaving 0.109moles fuel A total moles fuel = moles A + moles A2B5 moles A2B5 = 0.036moles B x (1A2B5 / 5B) = zero.0072moles A2B5 whole moles gas = 0.1162moles prior to the reaction, the pressure within the combined flask is: complete moles = 0.159moles mole fraction A = zero.123 / 0.159 = 0.774 mole fraction B = 0.036 / zero.159 = 0.226 when mixed, partial strain A + partial strain B = total strain (pressureA x mole fractionA + pressureB x mole fractionB) = new stress 1.5atm x zero.774 + zero.35atm x zero.226 = 1.24atm partial stress A + partial pressure A2B5 = complete strain mole fraction A after rxn = 0.109moles / 0.1162moles = 0.938 mole fraction A2B5 after rxn = zero.062 zero.938moles A x 1.24atm + 0.062molels A2B5 x 1.24atm = 1.24atm