Show caleulations for credit. Be mindful of significant figures. Using the follo

Question

Show caleulations for credit. Be mindful of significant figures. Using the following balanced equation for a reduction- oxidation reaction in an acidic solution, answer the following questions. 61.aq) + 14H.(ao + Cr2Oj2-(as) 3 las) + 2 Cr"(m) + 7 H,00) If the initial sample containing I had a mass of 3.653 g, and it required 32.47 mL of a 0.1251M Na Cr2O, solution to react fully, How many moles of Cr0 required? (6 pt.) were How many moles of I were in the sample? (6 pt.) How many grams of iodine were in the sample? (6 pt.) What was the % mass of 1 in the sample? (6 pt.)

Explanation / Answer

Moles of chromate ions required = Molarity*Volume = 0.1251*0.03247 = 0.004062

As per the reaction stoichiometry, 1 mole of chromate ion requires 3 moles of I- for complete reaction, so moles of I- in the sample = 6*Moles of chromate ion required = 6*0.004062 = 0.024372

Grams of iodide ion in the sample = Moles of I- * MW of I- = 0.024372*126.9 = 3.093

% of I in the sample = (Mass of I in the sample/Sample mass)*100 = (3.093/3.353)*100 = 92.25%

Hope this helps !

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