Each of the absorbance data values can now be converted into the concentration values by simply multiplying the absorban
Posted: Sat Jul 02, 2022 8:44 pm
- Each Of The Absorbance Data Values Can Now Be Converted Into The Concentration Values By Simply Multiplying The Absorban 1 (40.67 KiB) Viewed 17 times
- Each Of The Absorbance Data Values Can Now Be Converted Into The Concentration Values By Simply Multiplying The Absorban 2 (76.02 KiB) Viewed 17 times
- Each Of The Absorbance Data Values Can Now Be Converted Into The Concentration Values By Simply Multiplying The Absorban 3 (71.65 KiB) Viewed 17 times
2. Plot concentration on Y axis and time on the X axis. Fit a straight line through your data and display the equation for straight line and the linear regression (R²) value on the graph. Be sure to add a title to the chart and label the axes and upload the graph below.
Upload a snip of your graph here Concentration 0.5 0.45 0.4 0.35 0.3 0.25 0.2 0.15 0.1 0.05 0 image.png 11.41 KB 5 10 #15 15 Time (min) y = -0.0142x+0.3773 R² = 0.9284 20 25 30
Plot In (Concentration) on the Y-axis and time on the X-axis. Fit a straight line through your data and display the equation for straight line and the linear regression (R²) value on the graph. Be sure to add a title to the chart and label the axes and upload a snip of the graph below. In(Concentration) -0.5 -1 -1.5 -2 -2.5 -3 image.png 10.03 KB 5 10 #16 15 y = -0.0744x-0.8269 R² = 0.9988 Time (min) 20 25 30
Plot 1/Concentration on the Y-axis and time on the X-axis. Fit a straight line through your data and display the equation for straight line and the linear regression (R²) value on the graph. Be sure to add a title to the chart and label the axes and upload a snip of the graph below. 1/(Concentration) 16 14 12 image.png 12.2 KB 5 10 #17 15 y = 0.462x+0.8848 R² = 0.9606 Time (min) 20 25 30
# 18 # 19 Complete the table below using the information from the three graphs. Zero Order Plot First Order Plot Second Order Plot Edit Submit For Grading Correlation Coefficient (|R²|) B I S 3 Is the reaction zero order, first order, or second order with respect to crystal violet? How do you know? *Note: The correlation coefficient can be misleading. It is possible to have a high correlation coefficient (close to 1.0) in conjunction with data that is NOT linear. Thus you should never rely solely on the correlation coefficient as verification of linearity. Observation of the data (Does the graph look linear?) with the correlation coefficient is a better indication of linearity. TT 99 <> Slope = Does the graph appear to be linear? (yes/no) *If you're having trouble with copy/paste, try the "Choose File" button below. Choose File No file chosen Submit 0 n G unanswered not submitted No Retakes G unanswered not submitted No Retakes
# 20 # 21 What is the rate constant, k? Use the information from the equation of the straight line to answer this question. Be sure to include correct units for k. Report the value to 2 significant digits. Note: This constant is sometimes called a pseudo rate constant because it does not take into account the effect of the other reactant, hydroxide ion. √O 010 2 √0 % VO 0 Submit € ∞o →** ΦΩ] {B | DPB (D)ΠΙΣUIflime / > < ØB A. + EC ∞ ∞X1b ÷ Un TT A 1b TI √ 0 0² (0) Submit [0] € oo √0 d (0) [0] % VO 9, 101 (0) 9 101 (0) X + Write the correct rate law with respect to crystal violet for the reaction. «Ω]{5/ΠΒΙΠΕΙΣU/flim + 1 > ≤ Ø X ± E C ∞ UO IT - *. It - + ww BA BA 1b 1b TI - Fo... Siz... - - Fo... Siz... W ? W G unanswered not submitted No Retakes G unanswered not_submitted No Retakes
# 22 Calculate the half-life of the reaction. You can use the appropriate integrated rate equation or your graph. Show your work. Do not forget to include units.