how many moles of BaSO4 will form if 20.0 ml of 0.600 M BaC2 is mixed with 30.0 ml of 0.500 M MgSO4?
Molarity = number of moles / litres
This is a limiting reagent (LR) problem and you know that because amounts for BOTH reactants are given. I work these the long way.
BaCl2 + MgSO4 ==> MgCl2 + BaSO4
mols BaCl2 = M x L = ?
mols MgSO4 = M x L = ?
Use the coefficients in the balanced equation to convert mols BaCl2 to mols BaSO4.
Do the same and convert mols MgSO4 to mols BaSO4.
It is likely that the two values will not be the same which means one of them is wrong; the correct value in LR problems is ALWAYS the smaller value and the reagent responsible for that is the LR.
Use the smaller value for mols BaSO4 and convert to grams.
grams BaSO4 = mols BaSO4 x molar mass BaSO4.
thank you!
To determine the number of moles of BaSO4 that will form, we need to calculate the limiting reagent in the reaction between BaC2 and MgSO4.
Step 1: Calculate the number of moles of BaC2 in 20.0 mL of 0.600 M BaC2.
Moles of BaC2 = Molarity * Volume
Moles of BaC2 = 0.600 M * 0.0200 L = 0.012 moles
Step 2: Calculate the number of moles of MgSO4 in 30.0 mL of 0.500 M MgSO4.
Moles of MgSO4 = Molarity * Volume
Moles of MgSO4 = 0.500 M * 0.0300 L = 0.015 moles
Step 3: Determine the limiting reagent.
The limiting reagent is the reactant that is consumed completely, thereby limiting the amount of product that can be formed. The reactant that produces fewer moles of the desired product is the limiting reagent.
The balanced chemical equation for the reaction between BaC2 and MgSO4 is:
BaC2 + MgSO4 → BaSO4 + MgC2
From the equation, it can be seen that one mole of BaC2 produces one mole of BaSO4. Therefore, 0.012 moles of BaC2 will produce 0.012 moles of BaSO4.
From the equation, it can also be seen that one mole of MgSO4 produces one mole of BaSO4. Therefore, 0.015 moles of MgSO4 will theoretically produce 0.015 moles of BaSO4.
Since there is an excess of MgSO4 (0.015 moles) compared to BaC2 (0.012 moles), BaC2 is the limiting reagent.
Step 4: Calculate the number of moles of BaSO4 formed.
As determined in Step 3, the moles of BaSO4 formed is equal to the moles of BaC2.
Moles of BaSO4 formed = 0.012 moles
To find the number of moles of BaSO4 formed, we need to calculate the number of moles of BaC2 and MgSO4 first.
Step 1: Calculate the number of moles of BaC2:
Molarity of BaC2 = 0.600 M
Volume of BaC2 solution = 20.0 ml = 20.0 / 1000.0 L = 0.0200 L
Number of moles of BaC2 = Molarity * Volume
= 0.600 mol/L * 0.0200 L
= 0.0120 moles
Step 2: Calculate the number of moles of MgSO4:
Molarity of MgSO4 = 0.500 M
Volume of MgSO4 solution = 30.0 ml = 30.0 / 1000.0 L = 0.0300 L
Number of moles of MgSO4 = Molarity * Volume
= 0.500 mol/L * 0.0300 L
= 0.0150 moles
Step 3: Determine the limiting reactant:
To find the limiting reactant, we need to compare the number of moles of each reactant. The reactant that produces fewer moles of the desired product will be the limiting reactant.
From the stoichiometry of the balanced equation, we know that 1 mole of BaC2 produces 1 mole of BaSO4, and 1 mole of MgSO4 produces 1 mole of BaSO4.
Since the number of moles of BaC2 (0.0120 moles) is equal to the number of moles of MgSO4 (0.0150 moles), neither reactant is limiting.
Step 4: Calculate the number of moles of BaSO4 formed:
Since neither reactant is limiting, the number of moles of BaSO4 formed will be based on the stoichiometry of the balanced equation, which is 1:1 molar ratio with both BaC2 and MgSO4.
Therefore, the number of moles of BaSO4 formed will be equal to the number of moles of either BaC2 or MgSO4, which is 0.0120 moles.
Therefore, 0.0120 moles of BaSO4 will form.