An organic compound was synthesized and found to contain only c, h, n, o, and cl. it was observed that when a 0.150 g sample of the compound was burned, it produced 0.138 g of co2 and 0.0566 g of h2o. all the nitrogen in a different 0.200 g sample of the compound was converted to nh3, which was had a mass of 0.0238 g. finally, the chlorine in a 0.125 g sample of the compound was converted to agcl. the agcl, when dried, weighed 0.251 g. determine the empirical formula of this compound.

The number of moles is determined by the formula:

number of moles =

Now determining the number of moles:

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Molar mass of is

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Molar mass of is

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Molar mass of is

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sample contains . So,

of sample contains:

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Molar mass of is

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sample contains . So,

Now writing the formula with their respective moles:

Dividing with the smallest value of moles:

Hence, the empirical formula is .

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