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 stuck

185.0 mL of K₂Cr₂O₇ 0.600 M solution

Explanation:

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.

i would say b

explanation:

but i think i would need more information than that