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In a separate reaction, 0.775g of zinc powder was reacted with 8.5 ml of hydrochloricrnacid solution. The hydrochloric acid solution has a density of 1.09 g/ml. Use thisrninformation to answer the questions below.rnrnb. What is the limiting reactant? Which reactant is in excess?
Accepted Answer
b. To determine the limiting reactant, we need to calculate the number of moles of each reactant and compare them to their stoichiometric ratio.
For zinc (Zn):
Mass of Zn = 0.775 g
Molar mass of Zn = 65.38 g/mol
Number of moles of Zn = 0.775 g / 65.38 g/mol = 0.0118 mol
For hydrochloric acid (HCl):
Volume of HCl solution = 8.5 mL
Density of HCl solution = 1.09 g/mL
Mass of HCl solution = Volume × Density = 8.5 mL × 1.09 g/mL = 9.315 g
Assuming the HCl solution is 37% HCl (a common concentration for laboratory-grade HCl), we can calculate the mass of HCl in the solution:
Mass of HCl = 9.315 g × 37% = 3.46 g
Molar mass of HCl = 36.46 g/mol
Number of moles of HCl = 3.46 g / 36.46 g/mol = 0.0949 mol
Now we can compare the number of moles of each reactant to their stoichiometric ratio in the balanced chemical equation:
Zn + 2HCl → ZnCl2 + H2
From the equation, we see that the mole ratio of Zn to HCl is 1:2. Therefore, the number of moles of HCl required to react completely with 0.0118 mol of Zn is:
Number of moles of HCl required = 0.0118 mol × 2 = 0.0236 mol
Since we have only 0.0949 mol of HCl, which is less than the required 0.0236 mol, HCl is the limiting reactant. Zn is in excess.
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