Silver reacts in a single replacement reaction with 98.8 mL of 0.318 mol/L AuCl3. What mass of reducing agent is used.
To determine the mass of the reducing agent used in the reaction, we need to use the balanced chemical equation that represents the reaction.
The balanced chemical equation for the reaction between silver (Ag) and gold chloride (AuCl3) can be written as follows:
3Ag + AuCl3 -> 3AgCl + Au
From the balanced equation, we can see that the molar ratio between Ag and AuCl3 is 3:1. This means that for every 3 moles of Ag, we need 1 mole of AuCl3.
First, let's calculate the number of moles of AuCl3:
moles of AuCl3 = concentration of AuCl3 * volume of AuCl3 solution
= 0.318 mol/L * 0.0988 L
= 0.03149 mol
Next, let's calculate the moles of Ag:
moles of Ag = (moles of AuCl3) / (molar ratio with Ag)
= 0.03149 mol / 1
= 0.03149 mol
Finally, let's calculate the mass of Ag:
mass of Ag = moles of Ag * molar mass of Ag
= 0.03149 mol * 107.87 g/mol
≈ 3.392 g
Therefore, the mass of the reducing agent used in the reaction is approximately 3.392 grams.