Question

How many grams of each product result from the following reactions, AND how many grams of each reactant is left over? (Shntould be three amounts left over for each equation)

1) ( 1.3 g NaCl)+( 3.2 g AgNO3)→(xgAgCl)+(ygNaNO3)

2) ( 2.63 g BaCl2)+( 6.76 g H2SO4)→(xgBaSO4)+(ygH

Answer 1

(1) NaCl + AgNO3 → AgCl + NaNO₃

Molarmass of NaCl = 58.5 g/mol

Molar mass of AgCl = 143 g/mol

Molar mass of AgNO3 = 170 g/mol

Molar mass of NaNO3 = 85 g/mol

According to the balanced reaction,

1 mol=58.5 g of NaCl reacts with 1 mol=170 g of AgNO3

M g of NaCl reacts with 3.2 g of AgNO3

M = ( 3.2x58.5) / 170

    = 1.10 g of NaCl

So 1.3 - 1.1 = 0.2 g of NaCl left unreacted so it is the excess reactant.

Since all the mass of AgNO3 completly reacted it is the limiting reactant.

From the balanced reaction ,

1 mol=170 g of AgNO3 produces 1 mol=143 g of AgCl & 1 mol=85 g of NaNO3

3.2 g of AgNO3 produces X g of AgCl & Y g of NaNO3

X = ( 3.2x143) / 170                   and   Y = ( 3.2x85)/170

   = 2.7 g                                              = 1.6 g

Simillarly do the next one