2. A student performs the NaBH4 reduction of the triketone shown below (note that the equation is notproperly balanced). She starts with 1.20 grams of ketone and 0.130 g of NaBH4 and isolates 0.720 g ofproduct. Balance the equation and calculate the percent yield. Show your work.НОOHHPhPhNaBH4Ph+PhHHOH1.20 gMW: 238.240.130 gMW: 37.830.720 g isolatedMW: 244.29

Answered: Image /qna-images/answer/0b0cd746-b0f6-43bb-8926-75bee880165c.jpg

2. A student performs the NaBH4 reduction of the triketone shown below (note that the equation is not properly balanced). She starts with 1.20 grams of ketone and 0.130 g of NaBH4 and isolates 0.720 product. Balance the equation and calculate the percent yield. Show g of your work. HO OH Ph Ph NABH4 Ph Ph H OH H. 1.20 g MW: 238.24 0.130 g MW: 37.83 0.720 g isolated MW: 244.29

2. A student performs the NaBH4 reduction of the triketone shown below (note that the equation is not properly balanced). She starts with 1.20 grams of ketone and 0.130 g of NaBH4 and isolates 0.720 product. Balance the equation and calculate the percent yield. Show g of your work. HO OH Ph Ph NABH4 Ph Ph H OH H. 1.20 g MW: 238.24 0.130 g MW: 37.83 0.720 g isolated MW: 244.29

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

please check your answer. thank you!
An intern working in a research lab knocks over a beaker containing an important solution. The beaker originally contained 1.50 L of a 1.76 M solution, but after it spilled it only contained 0.95 L of solution. The intern decides to hide his mistake by refilling the beaker to contain 1.50 L again by adding pure water (not realizing that this will dilute the solution). What is the new concentration of the solution? Show all work and give your answer with three sig figs.
include oxidation reactions
Pre-lab: Theory The heat of neutralization of solid metal hydroxide with an aqueous solution of an acid might be determined directly in a one-step reaction МОН (:) + H M'+ Hә0(1) or indirectly using a two-step reaction MOH(s) - Mt + OH OH +H* → H2O(1) Based on the net ionic equation of the reaction, the theoretical enthalpy of reaction, AHneo kJ/mol], can be found from the enthalpies of formation as AHheo = AH; [H2O(1)] + AH; [M* (aq)] – AH¡ [MOH(s)] Based on the measured change in temperature, AT[K], and the heat capacity of the cup, Ccup[J /K], the experimental enthalpy of reaction, AHrp[kJ/mol], can be found as = - (Su Vtot + Ccup) AT/nL.R., where Vtot (mL] is the total volume of the solution, nL.R.[mmol] is the amount of the limiting reagent, and specific heat of water is s, = 4.18 JmL-'K-! The percent error can be found according to the formula ΔΗ 'exp AHiheo -AHiheo x 100% %E = Using the values for standard enthalpies of formation from the table 8-1 find the enthalpies for the…
Please solve for a and b
Please don't provide handwritten solution
I need help answering 4c.
I need help on this problem. And please only round off on the final answer.
R4
A pipet is used to transfer 5.00 mL of a 1.25 M stock solution in flask “S” to a 25.00-mL volumetric flask “B,” which is then diluted with DI H2O to the calibration mark. The solution is thoroughly mixed. Next, 3.00 mL of the solution in volumetric flask “A” is transferred by pipet to a 50.00-mL volumetric flask “B” and then diluted with DI H2O to the calibration mark. Calculate the molarity of the solution in volumetric flask “B.”
Please see screenshot and answer Questions 5 and 6 using the lab data given. Also, the enthalpy Magnesium oxide reaction is 1.18 kJ/mol and the enthalpy for the Magnesium reaction is 1.83 kJ/mol. Thank you!
i need help on this? this requries to check the soluble and insoluble charts