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%

1. Average number of moles in 100 mL for all three gases:
2. Percent Deviation for each gas:
3. Do your results confirm Avogadro's Law:

3. Based upon your experimental work, how many atoms of each substance are present? (There are 6.022 * 10^23 molecules/mole)

4. Even though the number of molecules can vary the conditions of pressure and temperature, the number of atoms in the gas at STP can vary depending on the gas. How many atoms are there in one molecule of methane, propane and butane?

5.  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 * 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 value for R (0.082057 L*atm/K*mol)

6. In a real gas (non-ideal gas) the molecules can interact with each other. If this interaction is attractive, how will the pressure value for this real gas be different than the calculation of pressure for an ideal gas?

Part 2: Please correctly answer the following Avogadros Law Laboratory questions

1. 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 * 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?

1. In this experiment, volume and temperature were held constant.  Which of the following relationships best describes the results of your experiment?  P = pressure, V=volume, n=number of moles, R=gas constant, T=temperature, and C=a constant

1. In a real gas (non-ideal), the molecules can interact with each other.  Suppose that the primary interaction between the molecules is attractive.  How would this affect the results?
2. In an ideal gas, P*V = n*R*T where P = pressure, V=volume, n=number of moles, R=gas constant, and T=temperature.  Consider a gas with pressure = 1 atm, 1 mole of molecules, and a temperature of 295 K.  R=0.082 atm*L/(mol * K).  How much volume should this gas occupy?  

1. Suppose you have 1 atm of gas A and 1 atm of gas B.  If A and B react to form C with a 1 A: 1 B: 1 C stoichiometry, what will the pressure of C equal?

1. Suppose you have 1 atm of gas A and 1 atm of gas B.  If A and B react to form C with a 1 A: 1 B: 2 C stoichiometry, what will the pressure of C equal?