Hi there i am having extreame difficulty doing pre lab homework can i please get help on the questions i have circled down below.

please solve the questions providing detailed solution so i can take notes and understand and better prepare for an actual lab

note-please provide details as you solve the problems so i can take notes too and learn please solve the questions curcled in red. Its only one red circle

**please solve the following problem so i can learn and understand from your answer

**I put a red curcle on the calculations question i want to learn .Solve them in step by step so i can learn from you.

**I have provided three imajes of the same worksheet but with better and clear imajes to help you .

**If information is unclear let me know .

*Determine the dry gas pressure for the butane gas.

*calculate the number of moles of butane gas .

*Determine the molar mass of the Butane gas.

*Compare your calculated molar mass to the actual molar mass of butane.

*Lastly just show me how i can write a nice conclusion on this lab .

thanks so much and ill leave a thumbs up :)

Determining the Molar Mass of Butane Purpose: To experimentally determine the molar mass of butane (CaH10). Materials: large beaker 100 ml graduated cylinder water . butane lighter electronic balance thermometer Procedure: 1. Fill the beaker % full with water. 2. Measure the temperature of the water. 3. Place the butane lighter under water. Remove and dry as thoroughly as possible. 4. Determine the mass of the butane lighter. 5. Fill the graduated cylinder to the top with water. Cover the top of the cylinder with a small piece of paper. Quickly invert and place the cylinder into the beaker taking care not to allow air into the cylinder. Remove the piece of paper. 6. Hold the butane lighter under the graduated cylinder. Depress the valve on the lighter to allow the butane gas to flow into the cylinder. 7. Allow approximately 50 mL of gas to enter the cylinder. Adjust the cylinder so the water level inside the cylinder is level with the water level outside the cylinder. Record the actual volume. 8. Thoroughly dry the butane lighter and then re-mass the lighter. Observations: Water and gas temperature 24.0C Atmospheric pressure 101.89 kPa Mass of the butane lighter Initial 15.24 Final 15.049 Volume of Butane gas 85.9 mb Calculations 1. Determine the dry gas pressure for the butane gas 2. Calculate the number of moles of butane gas 24.0C 101.89 kPa Water and gas temperature Atmospheric pressure Mass of the butane lighter Initial Final Volume of Butane gas 15.24 g 15.04 g 85.9 mL Calculations: Determine the dry gas pressure for the butane gas. Calculate the number of moles of butane gas. Determine the molar mass of the butane gas. Compare your calculated molar mass to the actual molar mass of butane. Conclusion: Write an appropriate conclusion Vapor Pressure of Water Temperature Pressure Temperature Pressure C Temperature { Press 06 09 11 21 22 5 IPad 25 2 2.0 30 12 42 58 24 10 12 888888888 10 30 18 21 40 Temperature (C) 0 Pressure (kPa) 0.6 0.9 1.1 12 1.4 1.6 1.8 2.1 23 8 10 12 Vapor Pressure of Water Temperature Pressure (C) (kPa) 21 2.5 2.6 23 2.8 24 3.0 25 3.2 26 3.4 27 36 38 29 4.0 Temperature ("C) 30 35 40 Pressure (kPa) 4.2 5.6 744 123 19.9 312 473 70.1 101.3 16 18 20 80 90 100