25 i got the #1, just not #2 and #3. an industrial chemical company has opened a new plant that will produce ammonia (nh3). hydrogen and nitrogen gases are reacted to produce the ammonia. for the first batch of ammonia production, 475 g of nitrogen is reacted with excess hydrogen, and 397 g of ammonia are produced. • write the balanced equation for the formation of ammonia from hydrogen and nitrogen. 3h2+n2--> 2nh3 • calculate the theoretical yield of ammonia. work must be shown to earn credit. • calculate the percent yield for the ammonia production. work must be shown to earn credit.

Answer :

Part (a) :  

Part (b) :  Theoretical yield of = 440.96 g

Part (c) : Percentage yield of ammonia is 90.03 %

Mass of = 475 g

Molar mass of = 28 g/mole

Molar mass of = 17 g/mole

Experimental yield of = 397 g

Part (a) :The balanced chemical reaction will be:

Part (b) :To calculate the moles of :

From the given balanced equation:

1 mole of gas produces 2 moles of

16.96 moles of gas produces moles of

Now we have to calculate the mass of

Therefore, the theoretical yield of gas = 440.96 g

Part (c) : Percentage yield :

Therefore, the % yield of ammonia is 90.03 %

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"

just did the assignment and the answer was #1 +2 n