I need help I don't get this
1. Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, Pbutane, alone. To do this, consult a reference and record the partial pressure of the water vapor, Pwater, at the temperature you recorded. Use the following formula to compute the partial pressure of the butane.
Pbutane = Atmosphere - Pwater
2. Use the following combined gas law formula and compute the volume that the butane sample will occupy at STP. (HINT: Convert both temperatures to Kelvin.)
Pbutane x Voriginal = Pstandard x Vfinal Troom Tstandard
3. Use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 L at STP.
Grams of butane you used “X” grams of butane mL of butane corrected to STP = 22,400 mL
4. Compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table.
5. Compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula:
% error = measured value - accepted value x 100 accepted value
Sure, I'd be happy to help you. Let's go step by step.
Step 1:
- Consult a reference to find the partial pressure of water vapor, Pwater, at the temperature you recorded.
- Record the value of Pwater.
- Use the formula Pbutane = Atmosphere - Pwater to compute the partial pressure of butane, Pbutane.
Step 2:
- Use the combined gas law formula: Pbutane x Voriginal = Pstandard x Vfinal x (Troom / Tstandard)
- Convert both temperatures (Troom and Tstandard) to Kelvin before using them in the formula.
- Compute the volume that the butane sample will occupy at STP.
Step 3:
- Use the ratio and proportion formula: (Grams of butane you used) / (mL of butane corrected to STP) = (22,400 mL) / (22.4 L)
- Solve for "X", which represents the grams of butane you need.
- Determine the mass of butane needed to occupy a volume of 22.4 L at STP.
Step 4:
- Calculate the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table.
Step 5:
- Compare your experimental results from Step 3 with the theoretical value from Step 4.
- Calculate the percent error using the formula: % error = (measured value - accepted value) / accepted value x 100.
I hope this helps! Let me know if you have any further questions.
I can help explain each step to you.
1. To determine the partial pressure of the butane, you need to know the partial pressure of the water vapor at the temperature you recorded. You can find this information in a reference source, such as a table or a handbook. Once you have the value for Pwater, you can use the formula Pbutane = Atmosphere - Pwater to calculate the partial pressure of butane (Pbutane), where Atmosphere represents the total pressure in the graduated cylinder.
2. The combined gas law formula relates the pressure, volume, and temperature of a gas. In this case, you want to compute the volume that the butane sample will occupy at STP (Standard Temperature and Pressure). You need to convert the temperatures to Kelvin by adding 273.15 to each of them. The formula is Pbutane x Voriginal = Pstandard x Vfinal x (Troom / Tstandard), where Pbutane is the partial pressure of butane from step 1, Voriginal is the initial volume, Pstandard is the standard pressure (usually 1 atmosphere), Vfinal is the final volume you want to calculate, Troom is the temperature in Kelvin of the room where the experiment was conducted, and Tstandard is the standard temperature at STP (usually 273.15 Kelvin).
3. The ratio and proportion formula is used to determine the mass of butane needed to occupy a specific volume at STP. The formula is "Grams of butane you used / X grams of butane = mL of butane corrected to STP / 22400 mL". You can rearrange this formula to solve for the unknown, which is the X grams of butane needed. Multiply the known values and divide by the unknown value on both sides of the equation.
4. To compute the theoretical molar mass of butane, you need to know the formula of butane (C4H10) and the atomic masses of carbon (12.01 g/mol) and hydrogen (1.008 g/mol). Multiply the number of carbon atoms by the atomic mass of carbon and the number of hydrogen atoms by the atomic mass of hydrogen. Then add those values together to get the molar mass of butane.
5. Finally, to calculate the percent error, you need to compare your experimental value from step 3 to the theoretical value from step 4. Subtract the experimental value from the theoretical value, divide the result by the absolute value of the theoretical value, and multiply by 100. This will give you the percent error.