An impure sample of zinc (Zn) is treated with an excess of sulfuric acid (H2SO4) to form zinc sulfate (ZnSO4) and molecular hydrogen (H2).

(a) Write a balanced equation for the reaction.

Zn(s) + →

(b) How many moles are in 3.70 g of pure zinc?

_ mol

(c) How many moles of hydrogen gas are formed if one mole of zinc is treated with excess sulfuric acid?

_mol

(d) If 3.70 g of pure Zn is treated with excess sulfuric acid, how many grams of hydrogen could be collected?

_ g

(e) If 0.0660 g of H2 is obtained from 3.70 g of impure sample, what is the percent purity of the sample?

_ %

Plzz a sample of table sugar (sucrose, c12h22o11) has a mass of 7.801 g. ● a) calculate the number of moles of c12h22o11 in the sample b) calculate the number of moles of each element in c12h22o11 (number of moles of c, number of moles of h & number of moles of o) in the sample. (use your answer from part a as your starting point.) show your work and highlight your final answer. calculate the number of atoms of each element in c12h22o11 (number of atoms of c, number of atoms of h & number of atoms of o) in the sample. (use your answers from part b as your starting for each element.) show your work and highlight your final answer.