In the texile industry, chlorine is used to bleach fabrics

Question

 

Any of the toxic chlorine that remains after the bleaching process is destroyed by reacting it with a sodium thiosulfate solution, Na2S2O3 (aq). 

 

Na2S2O3(aq)+4Cl2(g)+5H2O(l)=2NaHSO4(aq)+8HCl(aq)

 

If 142.35kg of Na2S2O3(aq) reacts with 50.12kg of Cl2 and 227.86kg of water, how many kilograms of NaHSO4 are expected?

 

Na2S2O3(aq) + 4Cl2(g) + 5H2O(l) = 2NaHSO4(aq) + 8HCl(aq)
1 4 5 2 8
142.35kg 50.12kg 227.86kg 42.62kg n/a
158.12g/mol 70.9g/mol 18.02g/mol 120.07g/mol n/a
0.900mol 0.71mol 12.64mol n/a
1/x = 4/0.71 1/0.900=4/y N/A 4/0.71=2/z
x=0.1775 y=2.7 z=0.355
EXC LIM

 

I think my answer is 42.62kg can someone check my answer? Not sure. 

 

Answer 1

I can't exactly follow your methodology, but the answer I get is 42.44 kg, so you answer seems close.  You and I should both check or calculations, and our molar masses. 

The limiting reactant is Cl₂, so I get 706.9 moles Cl₂ x 2 moles NaHSO4/4moles Cl₂ x 120.06 g/mole x 1kg/1000g = 42.44 kg NaHSO₄