1) Potassium hydroxide and phosphoric acid react to form potassium phosphate and

Question

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? (g)

(B) What is the starting mass of H3PO4? (g)

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. (g)

(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

(Show work for points)

Explanation / Answer

A) K3PO4 = 212g/mol

H3PO4 = 98g/mol

So there was 0.276mol of K or 15.456g KOH

And 0.276/3mol of H3PO4+86.8g = 95.816g H3PO4

B) 35g N2 = 1.25mol

with 5.8mol H2

N2 is the limitng agent

SO we get 1.25 * 2 = 2.5mol NH3 = 42.5g NH3

H2 left = 5.8 - 1.25*3 = 4.1g H2

C) 0.893/2 = 0.4456mol<0.519

NO is the limitng agent

NO2 produced is 0.4456mol

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