using the ideal gas equation date

CHEMISTRY/EXPERIMENTUSING THE IDEAL GAS EQUATIONNAME ___________________________________DATE ______________________PERIOD _____In this experiment a sample of butane gas will be collected from a commercial lighter by the waterdisplacement method. After correcting the data for a dry sample of the gas, the molar mass of butane canbe calculated by rearranging the ideal gas equation from PV = nRT.PROCEDURE:1. Record the room temperature, in degrees Celsius.2. Obtain a bucket with room temperature water.FLAME FROM LIGHTER = ZERO ON LAB3. Place a lighter under water in the bucket. Remove the lighter, shake off the water, and dry the outsidewith a tissue. Determine the mass of the lighter to the nearest 0.01 gram. Record.4. Completely fill a 100 mL graduated cylinder with water and invert in the bucket. Be careful not to let anyair into the cylinder.5. Release the butane gas from the lighter by pressing the small lever near the flint wheel. Release the gasunder water being careful that all of the butane is collected in the graduated cylinder by waterdisplacement. Release enough gas to fill the graduated cylinder between 80-90 mL.6. Allow the butane to reach room temperature (about 5 minutes). Adjust the level of the water inside andoutside the graduate until they are the same by raising or lowering the cylinder in the bucket. Thepressure from the gas is now equalized with atmospheric pressure.7. Read the volume of the gas collected using the cylinder's graduations (to the nearest 0.5 mL). Record.8. Remove the lighter from the bucket. Shake off any excess water, and dry with a tissue.Measure and record the mass of the lighter.PURPOSE: The purpose of this experiment is to determine the molar mass of butane gas using the ideal gasequation and to compare the experimental value with the theoretical value from the periodic table.DATA:Temp(room) °C KPressure(room) 758 mmHg kPaMass lighter(before)Mass lighter(after)gramsgramsVolume butane mL LVapor pressure water (P H2O ) 2.2 kPaANALYSIS/CALCULATIONS: (show calculations with complete units)1. Convert the room temperature from °C to K and add to the table above.2. Convert atmospheric pressure from mm of Hg to kPa and add to the table above.

3. Convert volume in mL to L and add to the table above.4. Determine the mass (in grams) of butane released from the lighter.5. Determine the partial pressure of dry butane gas. (P butane = P room - P H2 O ).6. Use the ideal gas equation to determine the moles of butane released.PV =nRT where R = 8.31 L kPamol K(Solve for n and use partial pressure of butane from #5 as pressure.)7. Use your experimental data (Do not use the periodic table.) to determine the molar mass of butane.(Remember molar mass = g/mol.)CONCLUSION/QUESTIONS:1. Butane has the formula C4H10. Determine the theoretical molar mass of butane.(Now use the values from the periodic table.)2. Calculate the % Error between your experimental value and the actual (theoretical) molar mass ofbutane.3. Can the same experimental techniques be used to determine the molar mass of all gases? Explain.(Hint: Butane is insoluble in water. What if the gas were soluble in water?)