Chemistry help?

[匿名]

2014-03-18 10:32 am

2C3H6(g) + 2NH3(g) + 3O2(g) → 2C3H3N(g) + 6H2O(g)

A 150.0 liter steel reactor at 25 ºC is filled with the following partial pressures of reactants: 0.500 MPa C3H6, 0.800 MPa ammonia, and 1.500 MPa oxygen gas.

a. What is the theoretical mass of acrylonitrile that can be produced from this mixture? The reactor is a closed vessel and its volume will not change. ( I have calculated this question already, but I don't know how to find b.)

b. If the reaction described in question part a proceeds to 90% yield, and no side reactions take place, what is the final total pressure in the reaction vessel at 400 ºC?

更新1:

But how about the 400 degree? Also can you show more clear about the step, because it is confusing to me. Thank you.

更新2:

Also, how can I calculate the mole of H2O?

回答 (1)

david

2014-03-18 3:23 pm

b. If the reaction described in question part a proceeds to 90% yield, and no side reactions take place, what is the final total pressure in the reaction vessel at 400 ºC?
For part (a) you should have used the ideal gas law to find the number of moles of each, used these to find the limiting reactant, then used that to find the theoretical yield of acrylonitrile.
Now calculate 90% of the theoretical yield as moles. Use this repeatedly to calculate 1st the moles H2O formed, then 2nd moles C3H6 used, and 3rd moles NH3 used, finally moles O2 used. Use the moles used of those 3 and subtract from moles of each from part (a) to get the excess (unreacted) number of moles of each. Add all these moles (90% of theoretical yield + water formed + ALL 3 excess reactants) and use the ideal gas law to convert the number of moles to a total pressure.

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