60g of solid Zn are added to 50mL of a 0.15M solution of HCl and undergo a chemical reaction according to the following equation: Zn(s) + 2 HCl(aq) ? ZnCl2(aq) + H2(g) a) How many grams of ZnCl2 can be produced from this reaction? b) How would you classify this reaction? As acid/base, oxidation/reduction or precipitation? c) Assuming that all the H2 that is produced in the reaction is taken to a different container, how much volume would it occupy under STP conditions? d) If the produced H2 is later mixed with 50g of F2 in balloon. What would be the partial pressure of F2 is the balloon is under 3atm of pressure? e) Pretend that the HCl of this reaction is used in the neutralization of 45mL of a solution of Ga(OH)3. What was the molarity of the Ga(OH)3 solution?