Please show all work. I have the solutions but I need to see the precise calcula

Question

Please show all work. I have the solutions but I need to see the precise calculations and methods. It will make sense if you show the calculations rather than just explain it in words. Thanks!

1.) In the following reaction run at 600 K, 4.5 moles of nitrogen gas are mixed with 11 moles of hydrogen gas:

N2(g) + 3 H2(g) -------> 2 NH3(g)

The reaction produces 6 moles of ammonia. How many moles of nitrogen gas remain?

2. When the following reaction is run, a 75% yield is achieved:

PCl3(g) + 3 NH3(g) -------> P(NH2)3 (g) -------> P(NH2)3 (g) + 3 HCl (g)

How many moles of phosphorous trichloride are required to produce 328 grams of HCl??

I know about percent yield, its actually pretty easy, but i dont know how to work backwards lol.

Explanation / Answer

1)

N2(g) + 3 H2(g) -------> 2 NH3(g)

For 6 moles of ammonia to be produced, N2 spent = No,of moles of NH3 /Stiochiometric coefficient of NH3 =6/2 = 3 moles.

then moles of nitrogen gas remain = 4.5-3 = 1.5 moles.

2)no.of moles in 328 gms of HCl = weight of HCl/Molecular weight of HCl = 328/36.5 = 8.9863 moles.

for 8.9863 moles of HCl to be produced, moles of phosphorous trichloride required = 8.9863/3 = 2.995 moles

for 75% yield, the moles of phosphorous trichloride required = 2.995/0.75 = 3.994 moles of PCl3

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