Editing Empirical Formula Notes
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<center><b>Empirical Formula Notes</b></center><br> <br> Definition:<br> <br> <br> <br> What does it mean?<br> <Br> <br> <Br> When do you have empirical formula:<br> <br> <br> <br> <u>Step to Calculate Empirical Formula</u><br> 1. Change mass percent (%) to actual masses or use given masses directly<br> *Assume 100.g compound (cpd) 2. Change mass of element to mole of element<br> <br> 3. Change moles to molar ratio.<br> *Take smaller mole number and divide this number into all other mole number.<br> 4. If all numbers are not whole, you need to determine a single number that you can multiple to all mole numbers so that the resultant number are <b>ALL WHOLE</b>.<br> *Need to determine which number. The key is the following decimal to fraction conversion. **1/6 (0.167) **1/5 (0.200) **1/4 (0.250) **1/3 (0.333) **2/5 (0.400) **1/2 (0.500) **3/5 (0.600) **2/3 (0.666) **3/4 (0.750) **4/5 (0.800) **5/6 (0.830) <br> --------------<br> <b>Example from board</b><br> <br> What is the Empirical Formula (EF) of the compound that is 25.9% nitrogen and 74.1% oxygen? (In other words, for N<sub>x</sub>O<sub>y</sub>, solve for x and y)<br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br> <br>
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