Write a flowchart

Procedures

$1.$ Fill a large beaker, plastic tray, or other large container with tap water. Fill a $100-$mL graduate cylinder with distilled water. Place the palm of one hand over the top of the filled cylinder, invert it$,$ and place it in the beaker or tray of water. Remove your hand. There should be no bubble for only a very small bubble$)$ at the top of the cylinder.

$2.$ Take a disposable lighter to the analytical balance. Tare the balance with a small sheet of paper on it$.$ Weigh the disposable lighter to the nearest milligram. Record its mass in your notebook. Hold the lighter by the small sheet of paper to avoid excess handling of the lighter.

$3.$ Take the disposable lighter out of the sheet of$10.$paper and hold it under the mouth of the$11.$inverted cylinder. Depress the lever on the lighter so that fuel escapes from the lighter but is captured in the inverted cylinder. Continue until the gas in the inverted cylinder is about an inch from its top. You will need to stop within the range of the volume markings on the cylinder.Remove the lighter and lay it on a dry towel or cloth.

$4.$ Hold the cylinder so that it is vertical and the levels of the water inside and outside are equal.Mark the level with your finger. Remove the cylinder. Determine the volume of the hydrocarbon that you just released.

$5.$ Wipe and shake as much water as practical from the disposable lighter without causing any more fuel to escape. Take the lighter back to the top$-$loader balance. Re$-$tare a small sheet of paper and weigh the lighter.

$6.$ Repeat Procedures $1$ through $5$ until you have four sets of data that you believe to be reliable. Do not count your first try at collecting gas. Vary the volume during each set of data; range from $50$ to $100$ mL of gas in your graduated cylinder. Your first set of data will probably not be consistent with the other sets of data.$)$

$7.$ Record the temperature of your water bath and the barometric pressure. Knowing the temperature of the water, you can go to tables such as the one below and determine the partial pressure due to water vapor. The barometric pressure at the time of the experiment will be equal to the partial pressure of the hydrocarbon plus the partial pressure of the water vapor if the water levels inside and outside the container were the same each time the volume was noted$).$

$8.$ Have your instructor sign your notebook and Report Form. Using your data set, complete the Report Form.