In the reaction between potassium dichromate (K2Cr2O7) and sulfur dioxide (SO2) in acidic solution, balance the equation and calculate the number of moles of potassium dichromate needed to completely oxidize 5 moles of sulfur dioxide to sulfuric acid (H2SO4).
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The balanced equation for the reaction between potassium dichromate and sulfur dioxide in acidic solution is:
K2Cr2O7 + 3SO2 + 4H2O → Cr2(SO4)3 + 2KHSO4
From the balanced equation, we can see that 1 mole of potassium dichromate reacts with 3 moles of sulfur dioxide.
To calculate the number of moles of potassium dichromate needed to completely oxidize 5 moles of sulfur dioxide to sulfuric acid, we need to use the stoichiometric ratio.
From the balanced equation, we have the following stoichiometric ratio:
1 mole of K2Cr2O7 : 3 moles of SO2
Therefore, if 3 moles of SO2 require 1 mole of K2Cr2O7, then 5 moles of SO2 will require (5/3) * (1 mole of K2Cr2O7) = 1.67 moles of K2Cr2O7.
Thus, 1.67 moles of potassium dichromate are needed to completely oxidize 5 moles of sulfur dioxide to sulfuric acid.
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