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    Ammonia is used to make nitric acid (HNO3) by the Ostwald Process.
    Three reactions occur in this process.
    Reaction 1 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
    Reaction 2 2NO(g) + O2(g) → 2NO2(g)
    Reaction 3 3NO2(g) + H2O(I) → 2HNO3(aq) + NO(g)
    5 (a) In one production run, the gases formed in Reaction 1 occupied a total volume of
    4.31 m3 at 25 ºC and 100 kPa.
    Calculate the amount, in moles, of NO produced.
    Give your answer to 3 significant figures.
    (The gas constant R = 8.31 J K–1 mol–1)
    ................................ ................................ .....
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    (Original post by we knnow)
    Ammonia is used to make nitric acid (HNO3) by the Ostwald Process.
    Three reactions occur in this process.
    Reaction 1 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
    Reaction 2 2NO(g) + O2(g) → 2NO2(g)
    Reaction 3 3NO2(g) + H2O(I) → 2HNO3(aq) + NO(g)
    5 (a) In one production run, the gases formed in Reaction 1 occupied a total volume of
    4.31 m3 at 25 ºC and 100 kPa.
    Calculate the amount, in moles, of NO produced.
    Give your answer to 3 significant figures.
    (The gas constant R = 8.31 J K–1 mol–1)
    ................................ ................................ .....
    i know how you work out the pv=nrt
    n = PV or 100 000 x 4.31
    8.31 x 298
    but what do you do next
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    Work out total mol of gases, then look at the products of rxn1 and see what proportion of all gases is NO.
 
 
 
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