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.
