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12 Dec 2019

Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas:


2NO(g) + O2(g)→ 2NO2(g)

In one experiment, 0.857 mol of NO is mixed with 0.498 mol of O2. Determine which of the two reactants is the limiting reactant. Calculate also the number of moles of NO2 produced.

Limiting reactant:



Moles of NO2 produced: _____ moles

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Related questions

Nitric acid (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas: 2NO(g) + O2(g) = 2NO2(g) In one experiment 0.889 mole of NO is mixed with 0.516 mol of O2.

a. Calculate also the number of moles of NO2 produced.

Please Help!

Thank You in Advance

1) Potassium hydroxide and phosphoric acid react to form potassium phosphate and water according to the equation.
 
        3KOH(aq)+H3PO4(aq)→K3PO4(aq)+3H2O(l)
 
Determine the starting mass of each reactant if 58.5g of K3PO4 is produced and 86.8g of H3PO4 remains unreacted.
 
(A) What is the starting mass of KOH? 
 
(B) What is the starting mass of H3PO4? 
 
2) Ammonia is produced by the reaction of nitrogen according to the equation.
 
         N2(g)+3H2(g)→2NH3(g)
 
(A) Calculate the mass of ammonia produced when 35.0g of nitrogen react with 11.6g of hydrogen. 
 
(B) Which is the excess reactant and how much of it will be left over when the reaction is complete?
 
3) Nitric axide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2) a dark brown gas:
 
       2NO(g)+O2(g)→2NO2(g)
 
In one experiment. 0.893 mol of NO is mixed with 0.519 mol of O2. Determnine which of the two reactants is the limiting reactant. Calculate also the number if moles NO2 produced.
 
(A) Limiting reactant
 
(B) moles of NO2 produced

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