Asked by Anonymous
A common laboratory preparation of hydrogen on a small scale uses the reaction of zinc with hydrochloric acid. Zinc chloride is the other product.
(a) If 13.0 L of H2 at 765 torr and 20.0 °C is wanted, how many grams of zinc are needed, in theory?
(b) If the acid is available as 8.59 M HCl, what is the minimum volume of this solution (in milliliters) required to produce the amount of H2 described in part (a)?
(a) If 13.0 L of H2 at 765 torr and 20.0 °C is wanted, how many grams of zinc are needed, in theory?
(b) If the acid is available as 8.59 M HCl, what is the minimum volume of this solution (in milliliters) required to produce the amount of H2 described in part (a)?
Answers
Answered by
DrBob222
Zn + 2HCl ==> H2 + ZnCl2
Use PV = nRT and solve for n = number of mols H2 at the conditions listed. Convert mols H2 to mols Zn, then
g Zn = mols Zn x atomic mass Zn.
b)
Convert mols H2 to mols HCl, then M HCl = mols HCl/L HCl. Solve for L and convert to mL.
Use PV = nRT and solve for n = number of mols H2 at the conditions listed. Convert mols H2 to mols Zn, then
g Zn = mols Zn x atomic mass Zn.
b)
Convert mols H2 to mols HCl, then M HCl = mols HCl/L HCl. Solve for L and convert to mL.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.