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The reaction is: Mg(s) + 2HCl(aq) --> MgCl2 (aq) + H2(g) 1. If 2.016 g of...

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Chemistry

The reaction is: Mg(s) + 2HCl(aq) --> MgCl2 (aq) + H2(g)

1. If 2.016 g of hydrogen (H2) was released, how many moles ofmagnesium reacted? How many grams of magnesium would this be?

2. How many moles of magnesium would replace one mole ofhydrogen (H) in the hydrochloric acid? How many grams? (This is theequivalent weight)

3. Compare the mass calculated above in question 2 to yourexperimental equivalent weight and calculate the percentdifference. What would cause your experimental value to bedifferent? %difference = [(calculated value-experimentalvalue)/(calculated value)]x100

4. Using the ideal gas law, calculate the value of R inL-atm/mol-K by assuming that an ideal gas occupies 22.4 L/mol atSTP.

Answer & Explanation Solved by verified expert
3.9 Ratings (416 Votes)
Mg 2HCl MgCl2 H2 1 Mass of hydrogen released 2016 g Molar mass of hydrogen 2 x 100794 gmol 201588 gmol Moles of hydrogen Mass of hydrogenmolar mass of hydrogen 2016 g201588 gmol 1000059 mol As Molar ratio of Magnesium and Hydrogen 11 in the above equation So    See Answer
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