Also, question 1 and 2. Coming from this experiment in case you need context Dat

Question

Also, question 1 and 2.
Coming from this experiment in case you need context
Data and Calculations moles of Al used mol weight of Al wire: (Show calculation setup.) theoretical yield (moles) of hydrogen This is also the volume of gas produced.) volume of water collected atmospheric pressure 7SB torr is is the total pressure of the gas mixture.) temp of the water: 2l ec -29l vapor pressure of water rb GSO torr (Read from a table in a reference book, at the water temperature.) (Subtract this value from the atmospheric P to obtain the pressure of dry hydrogen gas.) pressure of dry hydrogen torr This is the pressure of just the hydrogen; use this value in the PV nRT) Using PV nRT, calculate the moles of hydrogen produced: IO g mol (Show set-up.) (Make sure to use units consistent with the value of R you use.) Now calculate the error, using the actual moles obtained and comparing to the theoretical moles calculated from the moles of aluminum used. error actual moles theoretical moles x 100 theoretical moles Questions: 1. If the amount of gas collected had not been corrected for the presence of water vapor what effect would this have had on the calculated value of actual of hydrogen? 2. This experiment would also work using another reactive metal such as zinc. lf you had used the same number of grams of Zn s you did Al in this experiment, would you have obtained more or less hydrogen? Illustrate with an equation and calculation.

Explanation / Answer

Q1

if you do not correct for water pressure, which is about 18.65 mm Hg vs. 753.2 mm Hg

% error = (734.55-753.2 )/734.55*100 = 2.5389 % lower than real value

The moles will be 2.5389% more than the real value

Q2

MW of Zinc = 65.38 g/mol

MW of Aluminum = 26.981539 g/mol

clearly, if we use the same mas, then we will have LOWER amount of moles of Zinc, therefore, less reaction

Expect LESS products, that is, less H2

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