Experiment 8.docx

# Experiment 8.docx - Experiment 8 Analysis of Two –...

This preview shows pages 1–4. Sign up to view the full content.

Experiment 8: Analysis of Two – Component Alloy Bana Alani Chem 141-8966 Oct 8, 2016 Lab Notebook /6 Data/Log/Observations /3 Signature and Stamp /1 Procedure /2 Formal Report /59 Title Page /2 Objective /2 Data Summary/ Calculations /10 Discussion /15 Conclusion /6 Post lab questions /24 Computer Printout /35 Total /100

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Objective To determine the percentage of mass for each metal presents in a sample of zinc – aluminum alloy by combining stoichiometry and the Ideal Gas Law as follows: o Apply the Ideal Gas Law to determine the total number of moles of hydrogen gas produced by the reaction of zinc – aluminum alloy sample with hydrochloric acid solution. o Apply stoichiometry to determine the mass of each metal based on the calculated number of moles of hydrogen gas. Results and Calculations Table 1: Measurements Taken for Each Trial Measurements Trial 1 Trial 2 Mass of sample 4.7539 g 3.0699 g Water level difference (ΔH) 7.70 mmH 2 O 3.60 mmH 2 O Temperature of gas above the water 23.0 o C 23.0 o C Mass of water displaced by hydrogen gas 3093 g 2556 g Zn (s) + 2 HCl (aq) ZnCl 2 (aq) + H 2 (g) (Eq. 1) 2 Al (s) + 6 HCl (aq) 2 AlCl 3 (aq) + 3 H 2 (g) (Eq. 2) PV = nRT (Eq. 3) P bar = P H2O + P H2 ± P ∆h (Eq. 4) Since we were using zinc – aluminum alloy, then: mass Zn + mass Al = mass alloy
mass Al = mass alloy – mass Zn (Eq. 5) Both metals, Zn and Al, react with HCl solution and produce H 2 gas. mol H 2 from Al + mol H 2 from Zn = mol H 2 collected (Eq. 6) Based on the balanced chemical reactions between each metal and HCl solution (Eq. 1 and 2), we calculate the number of moles of H 2 gas produced by using stoichiometry as follows: mol H 2 from Zn = massZn× 1 mol Zn 65.382 g Zn × 1 mol H 2 1 mol Zn (Eq. 7) mol H 2 from Al = mass Al × 1 mol Al 26.982 g Al × 3 mol H 2 2 mol Al (Eq. 8) Substituting equation 5 into equation 8 gives: mol H 2 from Al = ( massalloy massZn ) × 1 mol Al 26.982 g Al × 3 mol H 2 2 mol Al (Eq. 9) The number of moles of H 2 gas produced by the alloy sample can also be calculated using the Ideal Gas Law as follows: n = PV RT (Eq.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

### What students are saying

• As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

Kiran Temple University Fox School of Business ‘17, Course Hero Intern

• I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

Dana University of Pennsylvania ‘17, Course Hero Intern

• The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

Jill Tulane University ‘16, Course Hero Intern