Given the balanced equation: H2 + Cl2 2 HCl ,
how many moles of HCl will be produced if 18.4 g H2 reacts with 127 g Cl2?
moles of H2=18.4/2=9.2moles
Moles of Cl2=127/72=less than 9.2
so the reaction is controlled by the amount of chlorine.
You will get twice the moles of HCl than you had of chlorine.
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To determine the number of moles of HCl produced, we need to apply stoichiometry, which is based on the balanced equation.
Step 1: Calculate the number of moles of H2 and Cl2.
To find the number of moles of H2, we will use the molar mass of H2, which is 2.016 g/mol:
Number of moles of H2 = Mass of H2 / Molar mass of H2
Number of moles of H2 = 18.4 g / 2.016 g/mol ≈ 9.12 mol
To find the number of moles of Cl2, we will use the molar mass of Cl2, which is 70.906 g/mol:
Number of moles of Cl2 = Mass of Cl2 / Molar mass of Cl2
Number of moles of Cl2 = 127 g / 70.906 g/mol ≈ 1.79 mol
Step 2: Determine the limiting reactant.
To identify the limiting reactant, we need to compare the mole ratios of the reactants to the balanced equation. According to the balanced equation, 1 mole of H2 reacts with 1 mole of Cl2 to produce 2 moles of HCl.
The mole ratio of H2 to Cl2 is 1:1, and the actual ratio found is approximately 9.12 mol H2 to 1.79 mol Cl2. The actual ratio of H2 to Cl2 is larger than the balanced equation ratio. Therefore, Cl2 is the limiting reactant.
Step 3: Calculate the number of moles of HCl produced.
Since Cl2 is the limiting reactant, the reaction will proceed based on its mole ratio to HCl. According to the balanced equation, 1 mole of Cl2 produces 2 moles of HCl.
Number of moles of HCl = Moles of Cl2 × Mole ratio of HCl to Cl2
Number of moles of HCl = 1.79 mol Cl2 × (2 mol HCl / 1 mol Cl2)
Number of moles of HCl = 3.58 mol HCl
Therefore, if 18.4 g of H2 reacts with 127 g of Cl2, approximately 3.58 moles of HCl will be produced.