A gas made up of homonuclear diatomic molecules escapes through a pinhole 1.07 times as fast as O2 gas. Write the chemical formula of the gas. Op

2. Run V (NH4)2S₂08 (mL) 20.00 20.00 10.00 5.00 20.00 15.00 1 2 3 4 5 6 [S₂082-] (mol/L) 0.04 0.04. 0.02 0.01 10.09 10.03. VKI (mL) 20.00 10.00 20.00 20.00 8.00 15.00 [1-] (mol/L) 0.08 0.07 0.08 0.08 0.032 V Na₂S₂03 (mL) 10.00 10.00 10.00 10.00 10.00 10.00 [S₂032-] (mol/L) 6.001 0.001 0.001 10.001 0.001 0.001 These calculated concentrations should be entered in the Data Table for this experiment for runs 1-6. To calculate the concentration of [12], use Equation (3) and the concentration of [S₂03²]. In a constant-temperature run described in the procedure section of this experiment, the solution turned blue in 50 s. a) Consider the concentration of [S₂032] in the mixed solution shown in the las column of the table from the previous exercise. Calculate the concentration c [12] final formed in this reaction. b) Calculate the rate of the reaction.

Data Analysis: 1. Create an Absorbance (Y) vs. Concentration (X) graph using data from the six standard solutions above. 2. Perform a linear trendline analysis of your six data points. Display the equation and R² value on the graph with a minimum of 8 decimal places. 3. On the same graph, perform a 2nd order polynomial trendline analysis of your six data points. Display the equation and R² value on the graph with a minimum of 8 decimal places. 4. Turn in your graph as the last page of this report. 5. On a separate piece of paper calculate the concentration of the unknown solution using both the linear and 2nd order polynomial trendline equations (Show all work) 6. Choose the best unknown concentration from #4 above and report it with three significant figures in the unknown data table above.

pH pH = 4.389 pH = 4.874 = pH = 5.339 pKa Answer Bank Using the equation to calculate the quotient [AT]/[HA] at three different pH values. [A] [HA] + log [A-] [HA] [A-] [HA] = = = LA I [HA] 1 0.3273

Determination of unknown acid concentration     Trial 1 Trial 2 Trial 3 Unknown Acid number Volume of acid used (mL) 25 mL 25 mL 25 mL Initial buret reading (mL) 50 mL 50 mL 50 mL Final buret reading (mL) 14.8 mL 15 mL 14.5 mL Volume of NaOH used (mL) 50 mL 50 mL 50 mL Molarity of NaOH       Calculated molarity of HCl (M)               Show a sample calculation of HCl molarity   AVERAGE MOLARITY OF Unknown HCl Show a sample calculation of NaOH molarity

How should number 2 be solved

7. Chemical Formula: C3H7NO₂ 1H, broad 12 10 2H, broad Final Answer 8 PPM 6 1H q A- 3H d 2 0

Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29   1.41   1.95   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 50.37   49.39   49.84 Table 2. Titration data   Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29   1.41   1.95   Molarity of NaOH (M) 0.100   0.100   0.100   Volume of vinegar sample (mL) 5.00   5.00   5.00   Final burette reading (mL) 50.37   49.39   49.84   Expected color at end point       Volume of NaOH used (mL) 48.08   47.98   47.89  Compute for the ff: a.   Average moles of acetic acid (mol)? b.  Average molarity of acetic acid (M)? c.  Average molarity of acetic acid (M)?