When Ammonia Burns In Oxygen At 800 C Over A Platinum Catalyst, The Products Are Nitric Oxide And Steam. The Equation For The Reaction Is 4 NH3(g) + 5 O2(g) ---> 4 NO(g) + 6 H2O(g), Can You Calculate The Volume Of Nitric Oxide That Is Produced If 1.20 X 10?

1.20 x 10^5 L of oxygen is used up in reaction.


Answer:
1 mole of a gas at STP is equal to 22.4 liters. So, 1.20 x 105 liters of oxygen means that x number of moles of oxygen are used:
x = 1.20 x 105/ 22.4
   = 5357 moles
Since 5 moles of oxygen produce 4 moles of NO, 5357 moles will produce:
(4 x 5357)/ 5 = 4285.6 moles
Hence, 4285.6 moles will be produced. To catch the volume of NO, simply multiply this by 22.4:
4285.6 x 22.4 = 9.6 x 104 liters (or dm3) ---ANSWER---




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