This is the stoichiometry from balanced equations in question 2&3 If I did like

Question

This is the stoichiometry from balanced equations in question 2&3 If I did like above picture.. Am I right? The triiodide produced by the first reaction is then consumed by the second one. Use the stoichiometry from the balanced equations in questions 2 and 3, to obtain the conversion factors for the overall reaction stoichiometry for this experiment. Complete the following dimensional analysis with the appropriate mol/mol ratios in the empty() positions shown mol S,O wel 13 :tration flock before it reacts

Explanation / Answer

Yes it looks right.

In the first reaction, 3 moles of I3- are produced from 1 mole of IO3-

In the second reaction, 2 moles of S2O32- react with 1 mole of I3- produced in first reaction.

Moles of S2O32-/L = Mole IO3-/L * (3 mol I3- / 1 mol IO3-) * (2 mol S2O32- / 1 mol I3-)

Conversion factor = 6

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