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

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter4: Chemical Reactions

Section: Chapter Questions

Problem 4.100P

See similar textbooks

Similar questions

Date:. Subject: in ine Production of aluminum sulfate from The Le llowing reaction: A1 O 3 + 3H₂2 504 if we Mix 8kgmol Al₂O3 and 40 H₂50₂4 Kgmal remains at the end of the reaction, it is desirable: Al find the excess Percentage of sulfuric acid. ●13) find the conversion Percentage of Al₂ oz. c) reaction efficiency in terms of Kg Al₂(SO4)3 Produced to kg A1₂03 input. molecular masses are as follows: A1 ₂ 0 ₂ = 102, H₂ 50₁-28, 1₂0, 18, Al₂(SO4) = 342 A1₂ (504)3 + 3H₂O 2 آذین بر CS Scanned with CamScanner
Consider the balanced reaction 4 A + 4 B → 5C+ 6 D. If 5.577 moles of C (MW = 36.53) are produced, how many grams of A (MW%3D 47.16) are consumed? Report your answer to three decimal places (ignore significant figures).
Pls do fast and i will rate instantly for sure Solution must be in typed form
8. A hydrocarbon fuel is fully combusted with 495.97 g of oxygen to yield 880.2 g of carbon dioxide and 396.34 g of water. A.) Find the empirical formula for the hydrocarbon. B.) The molecular formula of the hydrocarbon if its MW is 142.29 g/mol. 9. (5 points) The K, value of the reaction N₂O4 2NO₁₂ (g) ²(g) is 0.113. What is the Gibbs free energy, AG, of the reaction if the initial pressure of N₂O4 is 1.23 atm while NO₂ is 0.750 atm? Is the process spontaneous? 10. (5 points) The molar heat of vaporization of ammonia is 23.4 kJ/mol while its boiling point is -33.34 °C. Calculate the AS for the vaporization of 0.75 moles of ammonia. Express your answer with unit J/K.
REPOST please help with reaction 2 and 3 under calculations (for reaction 2 help had been provide till part 3 Note: Since you have posted a question with multiple sub-parts, we will provide the solution only to the first three sub-parts as per our Q&A guidelines. Please repost the remaining sub-parts separately. Given that: Initial temperature, T1 = 24.0oC Final temperature, T2 = 32.1oC Volume of HCl = 100 mL Density of HCl = 1 g/mL Concentration of HCl = 1.0 mol/L = 1.0 M arrow_forward Step 2 1.) The change in temperature is calculated using the following expression: ∆T=Final temprature-Initial temperature=T2-T1 Substitute 32.1oC for T2, and 24.0oC for T1 in the above expression to calculate the change in temperature for reaction 2. ∆T=32.1°C-24.0°C=8.1°C arrow_forward Step 3 2.) The formula to calculate the mass of a substance is written as follows: Mass=Volume×Density Substitute 100 mL for the volume and 1 g/mL for the density in the above formula to calculate the…
question 21 only please
(100g)(4.184J/g K)(t-22)=(275g)(0.444J/g K)(t-100) What is the step by step solution to this problem?
a) 4-Pentenoic acid + H, KMn04 / OH B 0-10°C NaBH4 b) CH,=CH-CH,-CH,-C -Co,H Mg Co c) 5-Chloro-1-pentene Etz0 Br2 Na,Cr0, d) Toluene CH;Br H3o*, heat F CyH-Bro Fe Na,Cr,0, H30*, heat
One of the best-selling light, or low-calorie, beers is 4.2%alcohol by volume and a 12-oz serving contains 110 Calories;remember: 1 Calorie = 1000 cal = 1 kcal. To estimatethe percentage of Calories that comes from thealcohol, consider the following questions. (a) Write abalanced chemical equation for the reaction of ethanol,C2H5OH, with oxygen to make carbon dioxide andwater. (b) Use enthalpies of formation in Appendix Cto determine ΔH for this reaction. (c) If 4.2% of the totalvolume is ethanol and the density of ethanol is0.789 g/mL, what mass of ethanol does a 12-oz servingof light beer contain? (d) How many Calories arereleased by the metabolism of ethanol, the reaction frompart (a)? (e) What percentage of the 110 Calories comesfrom the ethanol?
Esc ||| = OTHERMOCHEMISTRY A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). Calculating heat of reaction from bomb calorimetry data First, a 5.000 g tablet of benzoic acid (C6H,CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 16.00 °C to 38.96 °C over a time of 9.2 minutes. 2 4. Next, 5.730 g of acetaldehyde (C₂H₂O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 42.19 °C. 84°F Sunny Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: FI Explanation Is this reaction exothermic, endothermic, or neither? 4- F₂ Check 2C₂H4O(g) + 50₂(g) 4CO₂(g) + 4H₂O(g) Be sure any of your answers that are…
6.) Calculate the theoretical yield of the reaction below if 2.50 grams of reactant are used. Assume that the reaction proceeds via a 1:1 mole ratio. Show all work. OH MM-74.12 g/mol acid heat MM-56.11 g/mol 7.) How could IR be used to confirm the product above? Provide specific evidence.
Complete combustion of 5.50 g of a hydrocarbon produced 17.7 g of CO, and 6.03 g of H, O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. empirical formula: CH SPECIAL ΔΣΩ λμπ (s) (1) (aq) -> (g) () [ ] -> 1. CLR 3,438 19 SA stv W MacBook Air