25ml of NaCl was mixed with 10ml of AgNO3. A precipitate was made. What is the theoretical yield? What is the limiting and excess reagent?
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I think this problem has incomplete given. There is no data about the concentrations of NaCl and AgNO3. The concentration is usually in Molarity (mol/L) units.
Without it, you can't solve for the moles of each reactant species, and you can't determine the limiting/excess reactant.
To find the theoretical yield, limiting reagent, and excess reagent in this reaction, we first need to write the balanced chemical equation for the reaction.
The balanced chemical equation for the reaction between NaCl and AgNO3 is:
NaCl + AgNO3 -> AgCl + NaNO3
From the balanced equation, we can determine the stoichiometry of the reaction. The stoichiometric ratio in this reaction is 1:1, indicating that 1 mole of NaCl reacts with 1 mole of AgNO3 to produce 1 mole of AgCl.
Now let's calculate the number of moles of NaCl and AgNO3 given the volume of the solutions provided.
The molar concentration of a solution is calculated using the formula:
Molarity (M) = moles of solute / volume of solution in liters
Let's assume that the concentration of NaCl and AgNO3 solutions is given in moles per liter (M).
For the NaCl solution:
Volume = 25 mL = 25/1000 = 0.025 L
Concentration (NaCl) = 1 M
Moles of NaCl = Molarity * Volume
Moles of NaCl = 1 * 0.025
Moles of NaCl = 0.025 moles
For the AgNO3 solution:
Volume = 10 mL = 10/1000 = 0.01 L
Concentration (AgNO3) = 1 M
Moles of AgNO3 = Molarity * Volume
Moles of AgNO3 = 1 * 0.01
Moles of AgNO3 = 0.01 moles
Now, let's determine the limiting reagent. The limiting reagent is the reactant that is completely consumed first and limits the amount of product that can be formed.
Since the stoichiometric ratio is 1:1, the reactant with the fewer number of moles will be the limiting reagent. In this case, NaCl has fewer moles (0.025 moles) compared to AgNO3 (0.01 moles).
Therefore, NaCl is the limiting reagent.
To calculate the theoretical yield, we need to determine the moles of AgCl that can be formed using the limiting reagent.
From the balanced equation, we know that 1 mole of NaCl reacts to form 1 mole of AgCl.
The number of moles of AgCl formed is equal to the number of moles of the limiting reagent, which is 0.025 moles of NaCl.
Therefore, the theoretical yield of AgCl is 0.025 moles or the mass of AgCl can be calculated using its molar mass.
NOTE: To determine the limiting reagent and theoretical yield, we assume the reaction goes to completion and that there are no side reactions or losses during the process.