Consider the following chemical reaction. The equation is already balanced. Plea
ID: 998024 • Letter: C
Question
Consider the following chemical reaction. The equation is already balanced. Please show your work if you would like partial credit to be assessed.
4 NH3 + 5 O2 4 NO + 6 H2O
__________________ How many oxygen atoms are there in 15.00 grams of NO? Give the answer in moles.
__________________ What mass of oxygen is needed to react with 8.517 grams of ammonia?
__________________ How many moles of water are produced in a reaction in which 45.015 g of NO are produced?
__________________ How many grams of NO are actually produced when 60.02 grams of NH3 is allowed to react with 96.00 grams of oxygen? (This is a limiting reactant problem.)
Explanation / Answer
4 NH3 + 5 O2 4 NO + 6 H2O
1) 5 moles of oxygen will produces 4 moles of NO
in reverese 4 mole of NO produce by 5 mole of oxygen
no. of moles of NO = 15/30 =0.5 moles
therefore, 0.5 mole of NO will produce = 5/4 x0.5 mole of O2 = 0.625 moles.
2) 4 moles of NH3 will react with 5 moles of O2
no. of moles of NH3 reacted = 8.517/17 = 0.501 moles
therefore,
no. of moles of O2 reacted = 5/4 x 0.501 = 0.6262 mole
0.6262 mole of of O2 = 0.6262 x 32 grams of O2 = 20.04 grams
3) 4 moles of NO and 6 mole osf H2O are produced
no. of moles of NO = 1.5 moles
H2O produced = 6/4 x 1.5 = 2.25 moles
2.25 moles of H2O = 2.25 x 18 = 40.513 grams of H2O
4) 4 mole of NH3 will react with 5 mole of O2
No. of moles of NH3 = 3.53 mole
No. of moles of O2 = 3 moles
limiting reagent is NH3
therefore, NO produced = 106 grams (3.53 mole x 30)
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