Determine the mass in grams of oxygen present in the sample. Determine the numbe

Question

Determine the mass in grams of oxygen present in the sample. Determine the number of moles of nitrogen in the sample. Determine the number of moles of oxygen in the sample. The moles of
There are a number of steps involved in determining the empirical formula of a compound. You will need to demonstrate that you can complete all of these steps as you determine the empirical formula of a compound composed of nitrogen and oxygen that is 63.65 % N by mass. Complete your calculations based on 100 g of this compound. Enter all calculated values in 4 significant figures followed by one space and the appropriate unit. Use g for grams and mole for moles. Do not use scientific notation. Determine the mass in grams of oxygen present in the sample. Determine the number of moles of nitrogen in the sample. Determine the number of moles of oxygen in the sample. The moles of represents the smaller mole value. Write the empirical formula of the compound. You will not be able to show subscript values correctly. For example, H20 would be recorded for water.

Explanation / Answer

Let the mass of compound be 100 gms

Mass of Nitrogen in the compound = 63.65/100 * 100 = 63.65 gms

Mass Percent of Oxygen in the sample = 100% - 63.65% = 36.35%

Number of moles of Nitrogen in the sample = 63.65/14 = 4.546 moles

Number of moles of Oxygen in the sample = 36.35/16 = 2.27 moles

Hence there are 2 moles of Nitrogen for every one mole of Oxygen

Hence the moles of oxygen represents the smaller mole value

Empirical Formula of the compound = N2O

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