Asked by Bobby
How many mL of 3.84 M HCL are required to consume 4.12g of Zinc in the following reaction?
Zn(s) + 2HCL(aq)----> ZnCl2(aq) + H2(g)
Zn(s) + 2HCL(aq)----> ZnCl2(aq) + H2(g)
Answers
Answered by
DrBob222
A method to work all stoichiometry problems.
1. Write the equation and balance it. Your's looks ok.
2. Convert what you are given into mols. In this case, mols Zn = grams/atomic mass.
3. Using the coefficients in the balanced equation, convert mols Zn to mols HCl.
4. Now that you have mols HCl, remember mols = M x L. You have mols and M, calculate L and convert to mL.
Post your work if you get stuck.
1. Write the equation and balance it. Your's looks ok.
2. Convert what you are given into mols. In this case, mols Zn = grams/atomic mass.
3. Using the coefficients in the balanced equation, convert mols Zn to mols HCl.
4. Now that you have mols HCl, remember mols = M x L. You have mols and M, calculate L and convert to mL.
Post your work if you get stuck.
Answered by
Bobby
Your Steps made everything clear. Thank you so much :D
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