Calculate the limiting reagent : CaCl2 + 2AgNO3 → Ca(NO3)2 + 2AgCl ( 15.0mL of calcium chloride of a 0.050 mol/L was used ) and 20.0mL of a 0.10mol/L of silver nitrate solution was used
To determine the limiting reagent, we need to compare the moles of each reactant used.
Given:
CaCl2 concentration = 0.050 mol/L
Volume of CaCl2 used = 15.0 mL = 0.015 L
AgNO3 concentration = 0.10 mol/L
Volume of AgNO3 used = 20.0 mL = 0.020 L
First, calculate the moles of CaCl2 used:
moles of CaCl2 = concentration x volume
moles of CaCl2 = 0.050 mol/L x 0.015 L
moles of CaCl2 = 0.00075 mol
Next, calculate the moles of AgNO3 used:
moles of AgNO3 = concentration x volume
moles of AgNO3 = 0.10 mol/L x 0.020 L
moles of AgNO3 = 0.002 mol
According to the balanced equation, the stoichiometry of the reaction tells us that 1 mole of CaCl2 reacts with 2 moles of AgNO3 to produce 1 mole of Ca(NO3)2 and 2 moles of AgCl.
From the moles of CaCl2 and AgNO3 calculated above, we can see that there is an excess of AgNO3 (0.002 mol) compared to CaCl2 (0.00075 mol).
Therefore, CaCl2 is the limiting reagent in this reaction.