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B. Empirical Formula

CH 3. B. Empirical Formula. Smallest whole number ratio of atoms in a compound. C 2 H 6. reduce subscripts. B. Empirical Formula. 1. Find mass (or %) of each element. 2. Find moles of each element. 3. Divide moles by the smallest # to find subscripts.

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B. Empirical Formula

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  1. CH3 B. Empirical Formula • Smallest whole number ratio of atoms in a compound C2H6 reduce subscripts

  2. B. Empirical Formula 1. Find mass (or %) of each element. 2. Find moles of each element. 3. Divide moles by the smallest # to find subscripts. 4. When necessary, multiply subscripts by 2, 3, or 4 to get whole #’s.

  3. 1.85 mol 1.85 mol B. Empirical Formula • Find the empirical formula for a sample of 25.9% N and 74.1% O. 25.9 g 1 mol 14.01 g = 1.85 mol N = 1 N 74.1 g 1 mol 16.00 g = 4.63 mol O = 2.5 O

  4. N2O5 B. Empirical Formula N1O2.5 Need to make the subscripts whole numbers  multiply by 2

  5. STP • STP = Standard temperature and pressure • Where, • Temperature = 0°C = 273 K • Pressure = 101.3 kPa = 1 atmosphere (atm) • For ANY gas at STP, • 1 mol = volume of 22.4 L(molar volume) = 6.02 x 1023 particles of that gas

  6. Unit of density of a gas = g/L • Can be used to calculate the gram formula mass of that gas • Example 1: • Determine the volume of 0.600 mol of sulfur dioxide gas at STP

  7. More Examples • Determine the # of moles in 52.5 L of He gas at STP • Find the Number of Particles in 30 L of sulfur gas at STP • Find the mass of 43 L of nitrogen gas at STP

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