43.5g of chlorine gas reacted with 105.5g of silver to silver chloride. Determine the mass of the oxidizing reagent that reacts.
To determine the mass of the oxidizing reagent that reacts, we need to identify which reactant is being reduced and which reactant is being oxidized.
In this reaction, chlorine gas (Cl2) reacts with silver (Ag) to form silver chloride (AgCl). Since chlorine is gaining electrons and silver is losing electrons, chlorine gas is being reduced (it is the oxidizing reagent) and silver is being oxidized.
To calculate the mass of the oxidizing reagent (chlorine gas), we can use the stoichiometry of the reaction.
The balanced equation for the reaction is:
2 Ag + Cl2 -> 2 AgCl
From the equation, we can see that 1 mole of Cl2 reacts with 2 moles of Ag.
First, let's calculate the number of moles of Ag and Cl2 used in the reaction:
For silver (Ag):
molar mass of Ag: 107.87 g/mol
moles of Ag = 105.5 g / 107.87 g/mol = 0.977 mol
For chlorine gas (Cl2):
molar mass of Cl2: 2 * 35.45 g/mol = 70.9 g/mol
moles of Cl2 = 43.5 g / 70.9 g/mol = 0.613 mol
Next, let's determine the mole ratio between Ag and Cl2 from the balanced equation:
For every 2 moles of Ag, we need 1 mole of Cl2.
So, the mole ratio of Ag to Cl2 is 2:1.
Since 2 moles of Ag require 1 mole of Cl2, and we have 0.977 moles of Ag, we can calculate the moles of Cl2 required:
moles of Cl2 required = 0.977 mol Ag / 2 = 0.4885 mol Cl2
Finally, let's calculate the mass of the oxidizing reagent (chlorine gas):
mass of Cl2 = moles of Cl2 required * molar mass of Cl2
mass of Cl2 = 0.4885 mol * 70.9 g/mol = 34.64 g
Therefore, the mass of the oxidizing reagent (chlorine gas) that reacts is 34.64 grams.