Using the ideal gas law and stoichiometry calculations, determine the amount of zinc metal needed to produce 150 ml of h2 gas at 293 k via the oxidation reaction below

You did not include the reaction.

This reaction meets the statement:

Zn + 2 HCl ---> ZnCl2 + H2(g)

So, I am going to show you how to solve the problem ,from that reaction.

Data:
Zn =?
V = 150 ml
T = 293 k

I also have to assume atmospheric pressure, p = 1 atm

1) Determine the number of moles of H2 gas, using ideal gas law.

pV = nRT => n = pV / RT = 1 atm * 0,150 liter / (0,0821 atm*liter/K*mol * 293 k)

=> n = 0,0062 mol H2

2) State the molar ratios from the reaction:

1 mol Zn : 1 mol H2

3) State the proportion with 0,0062 mol H2

1 mol Zn / 1 mol H2 = x mol Zn / 0,0062 mol H2 =>

x = 0,0062 mol Zn

4) Determine the mass of Zn using the atomic mass of Zn: 65.39 g/mol

=> mass of Zn = 0,0062 mol * 65,39 g / mol = 0,41 g

0,41 g

Ibelieve your answer is true 

You use the atomic number to find out how many protons and neutrons there are in the atom. you use the atomic mass to find out how many protons and electrons there are in the atom.