A student is helping cleаn up the chemicаl supply clоset where humidity hаs caused the labels tо fall оff some of their containers. The supply closet contains two unknown canisters of gas. One is compressed helium, and one is compressed nitrogen, but without the labels it is unclear which is which. The student uses gas collection over water to determine the molar mass of the gas. Initial Mass of Gas Canister 93.230 Final Mass of Gas Canister 93.129 Mass of Gas Expelled from the Canister 0.101 Volume of Gas Collected 88.5 mL Water Temperature 22℃ Vapor Pressure of Water at 22℃ 0.0260 atm Atmospheric Pressure 1.013 atm Use the data in the table to determine the moles of the gas expelled from the canister. Use the data in the table to determine the molar mass of the unknown gas. Based on the data, is the unknown gas nitrogen or helium? If the student had failed to consider the vapor pressure of the water to find the corrected pressure of the gas, and instead used the atmospheric pressure, would the calculated value for the molar mass of the unknown gas be larger or smaller than the actual value? Explain. Gas collection over water works in this situation because both nitrogen and helium are mostly insoluble in water. If the unknown gas were very soluble, would the calculated value for the molar mass of the unknown gas be larger or smaller than the actual value? Explain. Show your work for all calculations. Note: Your answer(s) must be provided in this text box. If you are unable to show your work adequately using the Rich Text Editor, complete your work on scratch paper. Upload a photo of your work in the "Comments" of this exam immediately after you have completed and submitted the exam. You can access the "Comments" through the grade book. Answers on scratch paper alone will not be scored.