Click on the graph so that small black boxes show up on the outer borders of the graph. Right click to bring up a dropdo

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Click On The Graph So That Small Black Boxes Show Up On The Outer Borders Of The Graph Right Click To Bring Up A Dropdo 1 (73.35 KiB) Viewed 47 times

Click On The Graph So That Small Black Boxes Show Up On The Outer Borders Of The Graph Right Click To Bring Up A Dropdo 2 (59.95 KiB) Viewed 47 times

Click on the graph so that small black boxes show up on the outer borders of the graph. Right click to bring up a dropdown menu of options. Click "copy" to copy the graph and then "paste as picture" into a new document. This will then allow you to use the graph as an image so that you can print multiple graphs on one sheet. If you prefer to print each graph separately, when the black boxes are showing on the graph, it is all set to print out as a full-size page. Extracting Data from Excel Graphs Determining the order of the reaction with respect to crystal violet The graph from each set that gives the highest correlation coefficient, R is the one that is the best representation of the order of the reaction. This is the graph that corresponds to the order of the reaction with respect to crystal violet. The order of reaction with respect to the crystal violet should be the same for both concentrations of sodium hydroxide. If they differ significantly, contact your TA for help. Order of reaction with respect to crystal violet Correlation coefficient for 0.010M NaOH Correlation coefficient for 0.020M NaOH 0.9519 R²= 0.698 R²m Integrated rate equation for crystal violet The equation for a line is in the form of y=mx+b. Since the integrated rate equation is a linear relationship between time and some form of concentration, you can use the equation for the line that gives you the best R2 value as the integrated rate equation for that concentration. It must be slightly rewritten to be useful for your reaction. Use the following method to write the integrated rate equation that best fits your reaction. 1. Select the integrated rate equation given below that matches the order of reaction with respect to crystal violet that you chose based on your graphs. Order of reaction Integrated rate equation for the crystal violet/sodium hydroxide reaction [CV]=-kt+ [CV] 0.010 Zero order: In[CV]-kt+ In[CV] obte 1/ [CV] kt + 1/[CV] 0.020 First order: Second order: 2. Substitute the values in the line that correspond to the slope, k, and the intercept. For example, if you have a second order reaction with the following equation, y=0.089x+12000 you would use the equation for the second order reaction and substitute for k= 0.089M- imin-1 and the y intercept, (1/[CV]) = 12000. 3. Your integrated rate equation would then be 1/[CV] = 0.089t + 12000. This tailors the general integrated rate equation to match your data. Integrated rate equation for 0.020M NaOH: The slope of the line is the rate constant, k, for your reaction will vary based on the concentration of sodium hydroxide used. The remainder of the integrated rate equation will be the same for both concentrations of sodium hydroxide. Write the integrated rate equation for each experiment below. You may have slightly different intercepts due to error in your data. Integrated rate equation for 0.010M NaOH: COV=-2300.5+60163 1/[0] = 1x107 + + 2x10-5
Rate of reactions The slope of the integrated rate equation is the rate constant, k, for the crystal violet and is proportional to the rate of the reaction. You will have a different rate constant for each concentration of sodium hydroxide used since the increase in the sodium hydroxide increases the rate of the reaction. This increase in the value of the rate constant, k, is directly proportional to the rate of the reaction and can be used as a substitution for "RATE" in the rate law to find the order of reaction with respect to the sodium hydroxide. Rate constant, k, from the integrated rate equation for the 0.010M NaOH 01638 Rate constant, k, from the integrated rate equation for the 0.020M NaOH 2x10-5 Determining the order of the reaction with respect to sodium hydroxide Use the isolation method covered in experiment 1 and the rate law. RATE=k[CV] [OH-] to find the order of the reaction with respect to sodium hydroxide. Remember, you already have the order of reaction with respect to the crystal violet from the integrated rate equations generated earlier. The RATES used in the rate laws are the two calculated rates of reaction, k values, in the previous step. The order of reaction with respect to crystal violet was chosen earlier from the graphs with the highest correlation coefficient. Rate-KECU [Orgh Order of reaction for NaOH Determining the rate constant, k, for the rate law You now have all of the variables except k in the rate law above. Rearrange the rate law to solve for k using both concentrations of sodium hydroxide. The rate constants should be relatively close to one another. Average the two numbers to get a final value. Note: the value you get for this rate constant, k, IS NOT the same as the value from the integrated rate equation which is also labeled k. The value for k in the integrated rate equation assumes a given value for the sodium hydroxide concentration. The rate constant, k, in the rate law is independent of the sodium hydroxide equations. Rate law Rate constant for rate law Determining the overall rate law The general rate law is Rate= K[CV] [OH]. Fill in the orders of each reactant average rate constant found above into this equation. You now have an equation that allows you to monitor the rate of reaction for any combination of crystal violet and sodium hydroxide concentrations. 45