Determination of Ideal Gas Law Constant

Determination of Ideal Gas Law Constant Activity 1 If your concentration, moles, or R calculations are incorrect or your calculation work does not actually result in the desired final units or units are missing/incomplete or cancelled incorrectly, you will lose points. Be sure that every number you include has its associated unit. Email me if you are unsure or need assistance. Data Table 1 Trial 1 (1 mL H2O2) Trial 2 (1 mL H2O2) Trial 3 (2 mL H2O2) Trial 4 (2 mL H2O2) Trial 5 (3 mL H2O2) Trial 6 (3 mL H2O2) Trial 7 (4 mL H2O2) Trial 8 (4 mL H2O2) Air temperature (°C) 25°C 25°C 25°C 25°C 25°C 25°C 25°C 25°C Volume H2O2 liquid (mL) 1.0mL 1.0mL 2.0mL 2.0mL 3.0mL 3.0mL 4.0mL 4.0mL Initial Volume Gas (mL) 0.0mL 1.0mL 0.0mL 0.0mL 0.0mL 0.0mL 0.0mL 0.0mL Final Volume Gas (mL) 9.8mL 11.5mL 18.3mL 19.5mL 31.0mL 33.2mL 42.4mL 41.0mL ΔV (mL) 9.8mL0.0mL = 9.8mL 11.5mL1.0mL = 10.5mL 18.3mL -o.omL = 19.5mL -0.0mL = 31.0mL -0.0mL = 33.2mL -0.0mL = 42.4mL –0.0mL =42.4m 41.0mL -0.0mL = Question 1: Would the volume of oxygen that is generated be affected if a smaller mass of yeast were used? Why or why not? There would be a smaller amount of catalase present to perform as a catalyst to the decomposition of H2O2 resulting in a lesser amount of O2 produced. Activity 2 Data Table 2 Show work for determining Concentration of H2O2 in the box below. Concentration should be mol/L. Concentration H2O2 (mol/L) 30.0g H2O2/ 1000mL 30.0g H2O2 x 1.0mol H2O2 / 34.01g H2O2 = 0.88mols H2O2 / L Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Trial 6 Trial 7 Trial 8 1 mL H2O2 1 mL H2O2 2 mL H2O2 2 mL H2O2 3 mL H2O2 3 mL H2O2 4 mL H2O2 4 mL H2O2 Mole s H2O2 0.0009mol H2O2 0.0009mol H2O2 0.0018mol H2O2 0.0018mol s H2O2 0.0026mol s H2O2 0.0026mol s H2O2 0.0035mols H2O2 Mole s O2* 0.00045mol 0.00045mol s O2 s O2 0.0009mol s O2 0.0009mol s O2 0.0013mol s O2 0.0013mol s O2 0.00175mol s O2 0.00175mol s O2 0.0183L 0.0195L 0.031L 0.0332L 0.0424L 0.041L ΔV (L) 0.0098L 0.0105L *Hint: Use reaction stoichiometry to solve for moles of O2. Show work for determining moles of H2O2 for Trial 1 here: 1.0mL H2O2 x 1L/1000mL x 0.88mols H2O2/1L = 0.00088mols H2O2 Show work for determining moles of O2 for Trial 1 here: 0.0009mols H2O2 x 1.0mol O2/2.0mols H2O2 = 0.00045mols O2 Show work for determining moles of H2O2 for Trial 3 here: 2.0mL H2O2 x 1L/1000mL x 0.88mols H2O2/1L = 0.00176mols H2O2 Show work for determining moles of O2 for Trial 3 here: 0.0018mols H2O2 x 1.0mols O2/2.0mol H2O2 = 0.0009mols O2 Show work for determining moles of H2O2 for Trial 5 here: 3.0mL H2O2 x 1L/1000mL x 0.88mols H202/1L = 0.00264mols H2O2 0.0035mols H2O2 Show work for determining moles of O2 for Trial 5 here: 0.0026mols H2O2 x 1.0mol O2/2.0mols H2O2 = 0.0013mols O2 Show work for determining moles of H2O2 for Trial 7 here: 4.0mL H2O2 x 1L/1000mL x 0.88mols H2O2/1L = 0.00352mols H2O2 Show work for determining moles of O2 for Trial 7 here: 0.0035mols H2O2 x 1.0mol O2/2.0mols H2O2 = 0.00175mols O2 Insert a copy of your graph. Your graph must include the equation of the line displayed, your name and date in the title. You cannot complete the rest of this lab without this graph and the equation of the line. See the Week 6 Announcement for an example. Graph: Volume (L) O2 vs. Moles O2 Jacen Duplain 06/07/2021 0.05 0.04 f(x) = 23.64 x Volume (L) O2 0.04 0.03 0.03 0.02 0.02 0.01 0.01 0 0 0 0 0 0 Moles O2 0 0 0 0 0 Show work, including all units, for the calculations/conversions for Air Temperature, Gas Constant R and Percent Error in the boxes below. Calculations must include complete units to be correct. Air Temperature (K) Show work in the space provided. 25 + 273.15 = 298.15K Air Pressure (atm) Show work in the space provided. 29.85inHg * Equation of the Line = 0.9976atm Y = 23.64x Gas Constant R Show work in the space provided. Percent Error Show work in the space provided. Use 0.0821 L*atm/mol*K in your calculation 25.40mmHg∗1 atm 1 inHg 760mmHg 23.64 ( l ( 0.9976atm ) mols 298.15k = 0.0791 L∗atm mols∗ K ) L∗atm L∗atm −0.0791 | 0.0821 mol∗K mols∗ K | ∗100=3.65 %error 0.0821 L∗atm mol∗ K Question 2: Identify at least two potential sources of error in the experiment. Are any assumptions made that would add to the experimental error? Some potential sources of error would be the amount of gas that is lost between the time of adding H2O2 and securing the cap of the bottle. Another potential error source would be if any liquid is still in the container after rinsing the residual yeast from a previous trial.