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Dominik [7]
3 years ago
10

How many molecules of carbon monoxide (co) are needed to react with excess iron (iii) oxide (fe2o3) to produce 11.6 g of iron (f

e)?
Chemistry
1 answer:
Troyanec [42]3 years ago
7 0
<span>8.73 grams CO
   The balanced equation for the reaction is
3CO + Fe2O3 ==> 2Fe + 3CO2
   So for every 2 atoms of Fe produced, 3 molecules of CO is needed. So let's start by looking up the atomic weights of the involved elements:
 Atomic weight iron = 55.845
  Atomic weight carbon = 12.0107 
  Atomic weight oxygen = 15.999
   Molar mass CO = 12.0107 + 15.999 = 28.0097 g/mol
 Moles iron = 11.6 g / 55.845 g/mol = 0.20771779 mol
   Moles CO needed = 0.20771779 mol / 2 * 3 = 0.311576685 mol
 Mass CO needed = 0.311576685 mol * 28.0097 g/mol = 8.727169487 g Rounding to 3 significant figures gives 8.73 grams CO</span>
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Answer:

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Explanation:

Based on the reaction:

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<em>2 moles of NH3 react with 5/2 moles of O2 to produce 2 moles of NO.</em>

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To solve this question, we need to find the moles of each reactant in order to find the limiting reactant as follows:

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Using PV = nRT

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1atm*22.4L/0.082atmL/molK*273.15K = n

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For a complete reaction of 1.00 moles of NH3 are needed:

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The moles of NO produced are the same than moles of NH3 because 2 moles of NH3 produce 2 moles of NO. The moles of NO are 1.00 moles

And as 1.00moles of gas are 22.4L at STP:

<h3>The volume of NO is 22.4L at STP</h3>

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