Calculation Enter you calculated values into the provided table. Show one example of the calculation worked out below in

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Calculation Enter You Calculated Values Into The Provided Table Show One Example Of The Calculation Worked Out Below In 1 (41.53 KiB) Viewed 69 times

Calculation Enter You Calculated Values Into The Provided Table Show One Example Of The Calculation Worked Out Below In 2 (79.47 KiB) Viewed 69 times

Calculation Enter you calculated values into the provided table. Show one example of the calculation worked out below in the questions so that I can see your logic. Trial 1 2 3 4 mreactant 1.089 1.01 0.95 N/A molfe molo 0.019 moles mproduct- Mreactant 1.27-1.08 0-19 1.0h 1.15-LOR 55.945 +0.018.14 0.45 56.845 0.11=0-006875 11.06-0.95 0.0170 O.Odades Cilly ™ 0.007 mal N/A N/A 0.012mol 0.14 14 COX15 0.009 molfe/molo N/A Average (ratio) N/A
5. If the value of ratio is equal to a whole number (±0.2) then you know that the formula for iron (X) oxide must be FeOratio If, however, the value of ratio is equal to a decimal value outside the range above then the formula for iron (X) oxide must be Fe₂O (ratio 2). This is an oversimplification in some respects but will work for the experiment today. To fine tune the calculation you would need many more measurements and to precisely control the amount of oxygen in the system. Determine the empirical formula for Iron (X) oxide in your experiment and name the compound based on the inferred ionic state of Iron. Fe O Iron ( ) Oxide 6. Write the full balanced equation for the reaction, don't forget that the reactant oxygen is a diatomic element, and don't forget state functions. If asked by the instructor write the half reactions for the equation.