SOLVE ALL 7 QUESTION IN SEQUENCE PLEASE (IF
ADDITIONAL DETAILS NEEDED COMMENT BELOW)
Temperature of solution:
Room Temp runs = 23 Deg Celsius
High or low temp run initial temp = 16 Deg Celsius
High or low temp run final temp = 20 Deg Celsius
Solve All 7 Question In Sequence Please If Additional Details Needed Comment Below Temperature Of Solution Room Temp 1 (213.01 KiB) Viewed 47 times
Solve All 7 Question In Sequence Please If Additional Details Needed Comment Below Temperature Of Solution Room Temp 2 (197.18 KiB) Viewed 47 times
Lab Report: Kinetics of the Reaction of Crystal Violet and Sodium Hydroxide SOLVE LAB QUESTION 1-2-3-4-5-6-7 PLEASE, LET ME KNOW IF ANY ADDITION DATA NEEDED. Determination of Order of Reaction The rate of the reaction with respect to the coloured cation CV* is given below. Note that the negative sign is required because the crystal violet cation is a reactant which is consumed. A[CV] Rate= (4-3) At The rate law for the reaction is: Rate = k [CV*]* [OH-] (4-4) where k is the temperature-dependent rate constant, X is the reaction order with respect to CV*, and Y is the reaction order with respect to hydroxide ion, OH-. Rate = k [CV]*[OH-] = kps[CV*]* (4-5) where kps is the pseudo-rate constant when [OH-]. >> [CV*].. Kps = K[OH-] = k [OH-] (4-6) Combining equations 4-3 and 4-5 yields the following equation for rate. Rate=A[CV'] = kps [CV]x (4-7) At Applying calculus to this rate law yields the following integrated rate laws for each order of reaction. Note that third order is possible but extremely unlikely. Table 4-1: Dependence of Rate Law on Order Order of Reaction with Respect to CV* (X) 0 Slope of Linear Graph Integrated Rate Law (compare to y = mx +b) [CV*] =-kost + [CV*] In[CV*] =-kost + In[CV*] Linear Graphs to Confirm the Associated Order [CV*], versus t In[CV], versus t -kps 1 -Kps 2 1/[CV*] = kost + 1/[CV*] 1/[CV*], versus t kps Order with respect to hydroxide (Y) is determined by first taking the natural log of equation 4-6. In Kps = In (k [OH-].") (4-8) Invoking the mathematical rules of logarithmic functions gives the following 3 equations. In kps In k+ In [OH-]. (4-9) In Kps = In k + Y In [OH-]. (4-10) In Kps = Y In [OH-]. + In k (4-11) k = Ae-E/RT (4-12) Taking the natural log of both sides of the equation gives a form which is more easily graphed. Ink=- (7) +In A (4-13) R A graph of In k versus 1/T (in Kelvin) allows calculation of the activation energy of the reaction. Note that R= 8.3145 J mol¹¹ K-¹.
SOLVE LAB QUESTION 1-2-3-4-5-6-7 PLEASE, LET ME KNOW IF ANY ADDITION DATA NEEDED. 1. Use appropriate data and/or graphs to determine the order with respect to crystal violet. Explain your answer by referring to the graphs and equations as applicable. TABLE: 4-3: Summary of Data for Determination of X (Order with Respect to CV+) SOLUTION GRAPH SLOPE R^2 1 Abs Vs t -0.0281 0.9854 1 In(Abs) Vs t -0.0742 0.9996 1 1/Abs Vs t -0.2081 0.9748 2. Use appropriate data and/or graphs to determine the order with respect to hydroxide. Explain your answer by referring to the graphs and equations as applicable TABLE: 4-4: Summary of Data for Determination of Y (Order with Respect to OH-) Solution Calculted [OH-] Graph Plotted Slope R^2 1 0.01 In(Abs) Vst -0.0281 0.9854 2 0.005 In(Abs) Vs t -0.0313 0.9997 3 0.0025 In(Abs) Vst -0.0198 0.9981 3. Use appropriate data and/or graphs to determine the value of the rate constant, k, and its units. Explain your answer. 4. Write the complete rate law for the overall reaction. 5. Use appropriate data and/or graphs to determine the value of the activation energy, Ea. Explain your answer 6. Describe one prediction you can make about the reaction mechanism based on your determined rate law. 7. Use your experimentally derived rate law to calculate the initial rate of reaction for solution 1 at room temperature. Show your work. Repeat the calculation for solutions 2 and 3. Explain why the trend is observed.
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