A convenient laboratory source of hydrogen gas is the reaction of an aqueous hyd

Question

A convenient laboratory source of hydrogen gas is the reaction of an aqueous hydrochloric acid solution with aluminum metal. An aqueous solution of aluminum chloride is the other product of the reaction. How many grams of hydrogen are produced in the reaction between 12.5 g of aluminum and 250.0 mL of an aqueous hydrochloric acid solution that is 25.6% HCl by mass and has a density of 1.13 g/mL? A convenient laboratory source of hydrogen gas is the reaction of an aqueous hydrochloric acid solution with aluminum metal. An aqueous solution of aluminum chloride is the other product of the reaction. How many grams of hydrogen are produced in the reaction between 12.5 g of aluminum and 250.0 mL of an aqueous hydrochloric acid solution that is 25.6% HCl by mass and has a density of 1.13 g/mL?

Explanation / Answer

6HCl(aq) + 2Al(s) ----> 2AlCl3(aq) + 3H2(g)

No of mol of Al reacted = w/Mwt = 12.5/27 = 0.463 mol

mass of HCl solution = d*v

                     = 1.13*250

                     = 282.5 g
mass ofHCL present in solution = 282.5*25.6/100 = 72.32 g

No of mol of HCl present in solution = w/Mwt = 72.32/36.5 = 1.98 mol

6 mol HCL = 2 mol Al

Limiting reactant = Al

No of mol of H2 produced = 0.463*3/2 = 0.6945 mol

mass of H2 produced = 0.6945*2 = 1.389 g

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