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Draw the major organic product(s) for the following.
- You may assume each reaction occurs just one time.
- Show or depict any relevant stereochemistry in the products [R/S or E/Z labels are not needed].
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Solved in 2 steps with 1 images
- The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)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?(a) (b) (c) Br Br Nal acetone NaCN NaSCH 3
- A match is lit and held under a cold piece of metal. The followingobservations are made: (a) The match burns. (b) The metal getswarmer. (c) Water condenses on the metal. (d) Soot (carbon) isdeposited on the metal. Which of these occurrences are due tophysical changes, and which are due to chemical changes?+) b) H30 H2O6. Heat of Formation. Give the balanced chemical equation used to find the heat of formation of the following a) CH3COOH (1) b) Na2SO4(s)
- CH,CH,CI (5) ? AICI,While cooking, if the bottom of the vessels is getting blackened on the outside, it means that:(a) the fuel is not cooked completely.(b) the fuel is not burning completely.(c) the fuel is wet.(d) the is burning completely.3) How many liters of combusted propane (C3H8; 44 g/mol) are required to heat a 100 kg steel pipe (specific heat of steel is 0.420 J/g°C), from room temperature (20°C) to its melting point of 1300°C? The density of propane is 0.493 g/mL.C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH=–2220 kJ /mol 4) How much energy is required to produce 1.9 grams of glucose (C6H12O6; 180 g/mol) from CO2 and H2O. Use the following combustion equation to help you answer the question?6CO2(g) + 6H2O(l) → C6H12O6(s) + 6O2(g) ΔH= 2900kJ 19) What volume of 0.12 M Na2SO4 will be required to react with 35 mL of 0.05 M CrCl6? 24) In an experiment when 100 g of C3H8 is combusted, 30 g of carbon dioxide resulted. What was the percent yield for the reaction?
- 9 (b) please help asap28. Which of the following is true about the reaction? CH4 (s) + 20₂ (g) CO₂ (g) + 2H₂O + 393 kJ (a) 393 kJ of heat is released for five moles of CO₂ (g) produced. (b) This reaction is endothermic. (c) When 1 mole of C(s) reacts with 1 mole of O₂ (g), 393 kJ of heat is consumed. (d) This reaction is exothermic.31) H,O, H*, heat ?
