Ideal Gas Law

Name of the Experiment: Avogadro’s Law
Type Your Name:
Date: 11/17/13

Experiment 1
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1. For each gas, record the following: Propane Butane Methane a Name and formula C3H8 C4H10 CH4 b Mass of 100 mL gas (g) 0.274g 0.361g 0.100g c Molecular weight of the gas (g/mole) 44.10g/mol 58.12g/mol 16.04g/mol d Number of moles in the 100 mL sample 0.0062mol 0.0062mol 0.0062mol

Average of all 3 gases: (0.0062+0.0062+0.0062) / 3 = 0.0062

2. To verify Avogadro's Law, calculate the average number of moles for the three gases along with the percent deviation for each gas, according to the formula:

% deviation = |(moles of gas) - (average for all gases)| / (average for all gases) * 100%

%deviation= (0.0062 -0.0062) mol / 0.0062mol *100%

% deviation= 0%

a Average number of moles in 100 mL for all three gases 0.0062moles b % deviation for each gas All 3 the same: 0% c Do your results confirm Avogadro's Law? Yes

4. Based on the calculated number of moles in one 1 atm of gas, how many molecules are in 1 atm of gas? (There are 6.022 x 1023 molecules/mole)

Since all 3 gases have the same number of moles I will calculate 1 formula for all 3.
0.0062mol (6.022 x 1023 molecules/mol)= 0.0373364 →3.73 x 1022 molecules for each gas are in 1atm.

5. Even though the number of molecules in 1 atm of gas at constant pressure and temperature is identical, the number of atoms in the gas at STP can vary depending on the gas. How many atoms are there in one mole of methane (CH4)

1 mole of Methane CH4 = (6.022 x 1023 atoms/mole) = 6.022x1023 atoms of Methane in one mole

6. In this experiment, the pressure (P) was 1 atm, the temperature (T) was 295 K, the volume (V) was 0.150 L, and the number of moles (n)was 6.2 x 10-3 moles. The ideal gas law states that P*V = n*R*T. Based on your experiment, what value do you get for R? Is your value close to the standard