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A sample of 39.1 g of MnOâ‚‚ is added to a solution containing 45.3 g of HCl. What is the limiting reactant?

Answer :

Final answer:

After balancing the chemical equation and converting the given masses of MnOâ‚‚ and HCl to moles, it is determined that HCl is the limiting reactant as there are fewer moles of HCl available than required to fully react with the amount of MnOâ‚‚ present.

Explanation:

To determine the limiting reactant between MnOâ‚‚ and HCl, we must first write the balanced chemical equation for their reaction:

MnOâ‚‚ + 4HCl → MnClâ‚‚ + Clâ‚‚ + 2Hâ‚‚O

Next, we convert the given masses of the reactants to moles:

For MnOâ‚‚:

Molecular weight = 86.94 g/mol (Mn=54.94, O=16)

Moles of MnOâ‚‚ = 39.1 g / 86.94 g/mol

= 0.45 mol

For HCl:

Molecular weight = 36.46 g/mol

Moles of HCl = 45.3 g / 36.46 g/mol

= 1.24 mol

According to the stoichiometry of the balanced equation, the reaction requires 4 moles of HCl for every mole of MnOâ‚‚. Thus, to react with 0.45 mol MnOâ‚‚, we need:

0.45 mol MnOâ‚‚ x 4 mol HCl/mol MnOâ‚‚ = 1.8 mol HCl

Since we only have 1.24 mol of HCl, HCl is the limiting reactant.

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Rewritten by : Jeany

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