In the textile 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? Please show all your work!  

Answer 1

Seth, it's stoichiometry.  You have the balanced equation, so you can find the proper mole ratio.

 

Begin with the given:

 

142.35kg of Na2S2O3(aq)

 

convert to moles using molar mass;

 

142.35kg of Na2S2O3(aq) x 1000g/Kg x 1 mole/ 158.1 g = 900.38 moles

 

Use this to calculate kilograms of NaHSO4

 

900.38 moles Na2S2O3(aq) x 2 moles NaHSO4/ 1 mole Na2S2O3(aq) = 1800.76 mole NaHSO4

 

Repeat with each of the other reactants, Cl2 and H2O.  The reactant that produces the LEAST product is the limiting reactant (presumably it's not water...)

 

Use this reactant to finish by multiplying the number of moles of product by the molar mass of the product to get the mass produced of the product.  

 

Can you take it from here?