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- Salicylic acid and ethanamide were made to react in basic medium to produce aspirin and substance X. A chemist is doing a research regarding the synthesis and have seen in scientific references that the process would produce an expected amount of 8.6 grams of aspirin at 74.2% efficiency given the right condition and amount of starting material: Density Ethanamide: 1.16g/mLA. What is the probable identity of Substance X? B. How much (grams) of substance X is produced? C. How many grams of Salicylic acid was used? D. How many grams of ethanamide should be used? E. What volume of excess ethanamide must be taken from the stock ethanamide solution? F. Show the mechanism of the reaction. OWN SOLUTION AND ANSWER ALL FOR UPVOTESalicylic acid and ethanamide were made to react in basic medium to produce aspirin and substance X. A chemist is doing a research regarding the synthesis and have seen in scientific references that the process would produce an expected amount of 8.6 grams of aspirin at 74.2% efficiency given the right condition and amount of starting material: Density Ethanamide: 1.16g/mLA) What is the probable identity of Substance X?B) How much (grams) of substance X is produced?C) How many grams of Salicylic acid was used?OWN SOLUTIONS AND NOT AI FOR UPVOTEA spray can is used until it is empty except for the propellant gas, which has a pressure of 1344 torr at 23 °C. If the can is thrown into a fire (T = 475 °C), what will be the pressure in the hot can? Please show steps
- 10 mol of NH3 (g) were placed in a previously evacuated 20-L container. After a sudden temperature rise to 961.4 K, 80% of ammonia dissociated into hydrogen and nitrogen according to the reaction: 2/3 NH3 (g) --> 1/3 N2 (g) + H2 (g) What is the total pressure of the mixture if all gases are ideal? (Answer in sig figs)The combustion of glucose produces carbon dioxide and water according to the unbalanced reaction below. C6H12O6 (s) + O2 (g) rightwards arrowCO2 (g) + H2O (g) If 0.479 g of glucose is added to a 110.24 mL container containing 1.63 atm O2 at 157ring operatorC, how many moles of H2O are produced? Report your answer in scientific notation.In Ammonia production, a reactor is supplied with a feed of 100L of N2 and 400L of H2 both at 22 atm and4200C. If the reaction is 95% complete (base on limiting reactant):a. Which is the limiting reactant?b. What is the number of moles of H2 remaining after the reaction?c. What is the number of moles of N2 remaining after the reaction?d. What is the percent conversion of N2?e. What is the number of moles of NH3 after the reaction?
- Some fire extinguishers spray gas pressure generated by the reaction of baking soda with sulfuric acid: NaHCO3(aq)+H2SO4(aq)-->CO2(g)+NaHSO4(aq)+H2O(l). Predict the pressure (atm) that could build up in a 25.0L tank if 1750.0g NaHCO3 reacted with excess H2SO4 at 35 degreesSucrose (C₁₂H₂₂O₁₁) ferments to alcohol and carbon dioxide according to the reaction: C₁₂H₂₂O₁₁ (s) + H₂O (l) —> 4 C₂H₅OH (aq) + 4 CO₂ (g) What mass of sugar would be required to produce 34.3 L of CO₂ at 50 °C collected over water at a total pressure of 795 mm Hg? The following molar masses MAY be helpful C₁₂H₂₂O₁₁ 342.3 g/mol H₂O 18.02 g/mol C₂H₅OH 46.07 g/mol CO₂ 44.01 g/mol The vapor pressure of water at 50 °C is 92.5 mm Hg.15.3 g of KClO3 decomposes according to the following reaction. Determine the volume of O2 formed at 1 atm and 500K. Show work for credit. The molar mass for KClO3 is 122.55 g/mol. 2 KClO3(s) → 2 KCl(s) + 3 O2(g)
- Ethanol (C2H5OH) burns in air according to the equation: C2H5OH + 302 > 2002 + 3H20 Determine the volume of O2 (in liters) at 35°C and 790 mm Hg required to burn 2.0 moles of ethanol.When 1.45atm of H2 reacts with 1.88atm of O2 in a 33.00L container at 25C, how many of H2O are formed? Express with right amount of sig figs3. Propane(C3H8) burns in oxygen to produce CO2 and water C3H8 + 5O2 → 3 CO2 + 4H2O (a) How many moles of oxygen are required to burn 4 moles of propane? (b)Calculate the moles of CO2 produced (c) Calculate the volume of CO2 produced by burning of 5moles propane at rtp (d) How many moles of water is produced (e) Calculate the mass in grams of water produced