An organic compound is 61.5% C, 2.56% H and 35.9% N by mass. 2.00 grams of this gas is entered into a 300.0 mL flask and heated to 228 degrees C. At these conditions, the gas exerts a pressure of 2670 torr. Find the empirical formula.

C₄H₂N₂

Explanation:

First we calculate the moles of the gas, using PV=nRT:

P = 2670 torr ⇒ 2670/760 = 3.51 atm

V = 300 mL ⇒ 300/1000 = 0.3 L

T = 228 °C ⇒ 228 + 273.16 = 501.16 K

Now we calculate the molar mass of the compound:

Finally we use the percentages given to calculate the empirical formula:

So the empirical formula is C₄H₂N₂

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