Given the balanced equation for the oxidation of ethanol, C2H5OH, by potassium dichromate:

3 C2H5OH + 2 K2Cr2O7 + 16 HCl → 3 C2H4O2 + 4 CrCl3 + 4 KCl + 11 H2O

calculate the volume of a 0.600M K2Cr2O7 solution needed to generate 0.1665 moles of C2H4O2 from a solution containing excess ethanol and HCl

need help stuck

Having the equation balanced in the statement, it is calculated based on the stoichiometric ratio of it, how many moles do I need from K₂Cr₂O₇ to be able to generate 0.1665 moles of C₂H₄O₂

3 moles C₂H₄O₂ _____ 2 moles K₂Cr₂O₇

0.1665 moles C₂H₄O₂ _____ X = 0.111 moles of K₂Cr₂O₇

Calculation: 0.1665 moles x 2 moles / 3 moles = 0.111 moles of K₂Cr₂O₇

Now the volume of solution of K₂Cr₂O₇ that contains the amount of moles calculated above is calculated, as stated in the molar concentration (0.600M), it is calculated:

0.600 moles of K₂Cr₂O₇ _____ 1000 mL solution

0.111 moles of K₂Cr₂O₇ _____ X = 185.0 mL of solution

Calculation: 0.111 moles x 1000 mL / 0.600 moles = 185.0 mL of solution

Therefore, to generate 0.1665 moles of C₂H₄O₂, 185.0 mL of K₂Cr₂O₇ 0.600 M solution is needed.