What is the volume in milliliters of 0.1069 M Cr2O72- required to react with 252.4 mL of 0.08013 M Cl- according to the reaction below?
6 Cl-(aq) + Cr2O72-(aq) + 14 H+(aq) ® 3 Cl2(g) + 2 Cr3+(aq) + 7 H2O(l)
mols Cl^- = M x L = ?
Using the coefficients in the balanced equation, convert mols Cl^- to mols Cr2O7^2- and that is mols Cl^- x 1/6 = ?
The M Cr2O7^2- = mols/L. You know M and mols, solve for L and convert to mL.
To find the volume in milliliters of the Cr2O72- solution, we need to use the concept of stoichiometry.
First, let's determine the balanced equation for the reaction:
6 Cl-(aq) + Cr2O72-(aq) + 14 H+(aq) ® 3 Cl2(g) + 2 Cr3+(aq) + 7 H2O(l)
From the balanced equation, we can see that the ratio of Cl- to Cr2O72- is 6:1. This means that for every 6 moles of Cl- required, 1 mole of Cr2O72- is needed.
Now, we can use this ratio to calculate the moles of Cl- in the solution:
Moles of Cl- = Volume of Cl- solution (in liters) * Molarity of Cl-
Convert the given volume of Cl- solution to liters:
Volume of Cl- solution = 252.4 mL * (1 L / 1000 mL) = 0.2524 L
Now, calculate the moles of Cl-:
Moles of Cl- = 0.2524 L * 0.08013 M = 0.02025 moles
According to the balanced equation, the mole ratio of Cl- to Cr2O72- is 6:1. Therefore, the moles of Cr2O72- required can be calculated using this ratio:
Moles of Cr2O72- = (Moles of Cl-) / 6 = 0.02025 moles / 6 = 0.003375 moles
Finally, to find the volume of the Cr2O72- solution in milliliters, we can use the formula:
Volume of Cr2O72- solution (in mL) = Moles of Cr2O72- * Molarity of Cr2O72- / (Molarity of Cr2O72- * 1000)
Given: Molarity of Cr2O72- = 0.1069 M
Volume of Cr2O72- solution = 0.003375 moles * (0.1069 M / (0.1069 M * 1000)) = 31.69 mL
Therefore, the volume in milliliters of the 0.1069 M Cr2O72- solution required to react with 252.4 mL of the 0.08013 M Cl- solution is 31.69 mL.