Data Analysis 2 How many moles of silver nitrate were added to the reaction? n = mass / molar mass mass after adding 200 mL of silver nitrate = 390.2339-185.000g = 205.2339 molar mass of silver nitrate = 169.87 g/mol n = 205.233/169.87 = 1.20 moles ??] ???EEE??] Conclusions 3. Did all the silver ions get consumed in the reaction? The molar mass of silver is 107.87 g/mol. Justify your answer.
The Correct Answer and Explanation is :
To address the given questions, let’s compute the correct values and explanations systematically.
1. Moles of Silver Nitrate Added to the Reaction
The moles of silver nitrate ((n)) are calculated using the formula:
[
n = \frac{\text{mass}}{\text{molar mass}}
]
Calculation:
- Mass of silver nitrate = (390.2339 \, \text{g} – 185.000 \, \text{g} = 205.2339 \, \text{g})
- Molar mass of silver nitrate (( \text{AgNO}_3)) = (169.87 \, \text{g/mol})
Substitute into the formula:
[
n = \frac{205.2339}{169.87} \approx 1.21 \, \text{moles}
]
Thus, 1.21 moles of silver nitrate were added.
2. Did All Silver Ions Get Consumed in the Reaction?
To determine whether all the silver ions (( \text{Ag}^+ )) were consumed, additional details such as the stoichiometry of the reaction, the limiting reactant, and the amount of the other reactants/products are necessary. However, the question prompts us to examine this through the molar mass and justification.
Molar Mass of Silver (( \text{Ag} )):
The molar mass of silver (( \text{Ag} )) is (107.87 \, \text{g/mol}).
If 1.21 moles of silver nitrate were added, (1.21 \, \text{moles}) of ( \text{Ag}^+ ) ions are available since each mole of silver nitrate provides one mole of ( \text{Ag}^+ ). If the reaction’s stoichiometry requires equal or fewer moles of ( \text{Ag}^+ ) than reactant molecules, all the silver ions are consumed.
Justification:
Assuming no residual silver was left (observed as a precipitate or unreacted ions in solution), the reaction consumed all ( \text{Ag}^+ ). However, if there’s residual solid silver or unreacted ( \text{Ag}^+ ) in the solution, then not all ( \text{Ag}^+ ) ions were consumed.
If ( \text{Ag}^+ ) ions fully reacted:
[
\text{Mass of silver produced} = n \times \text{Molar mass of Ag} = 1.21 \times 107.87 \approx 130.52 \, \text{g}
]
If observed silver product mass matches this value, all ( \text{Ag}^+ ) ions were consumed. Discrepancies indicate incomplete reaction.
Conclusion:
- ( \text{1.21 moles} \, \text{of AgNO}_3 ) were added.
- Whether all ( \text{Ag}^+ ) ions were consumed depends on reaction stoichiometry and product mass.