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Q: Question attached
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- Acetic acid (CHaCOOH) can be produced based onthe reaction: CHgCOOC2H5+ H20+CH COOH+C2H5OH. If there are 344.5 g of CHgCOOC2H5 and165.8 g of H20a. How many moles of acetic acid will be produced?3.910 b. Calculate the percent yield if 125 g of acetic acidwas produced (express your answer in 1 decimal placeonly).53 2How many moles of aluminum oxide are produced according to the reaction below, given that you start with 19.0 grams of Al and 12.0 grams of O2?Reaction: 4Al + 3O2 → 2Al2O3 A) 0.222 B) 0.185 C) 0.741 D) 0.250 E) not enough information Group of answer choices A B C D EGiven the following reaction. 2Na2S + __Na2CO3 + __SO2(g) __Na2S2O3 + CO2(g) DH =-1025kJ A. Balance the above equation by filling in the missing coefficients. B. Provide the name of Na2CO3. C. How many grams of CO2(g) would be produced if 12.5g SO2(g) reacted with 10.0g Na2S. Assume Na2CO3 is in excess.
- How many moles of C6H12O6 are formed when 7.46 moles of O2 are produced in the following reaction ? (answer to 2 decimal places). 6 CO2 + 6 H2O → C6H12O6 + 6 O2Given the following Reaction: 2C5H10O2 + 13O2 → 10CO2 + 10H2O. If 3.95 moles of O2 are reacted with an EXCESS of C5H10O21. a. a. How many moles of C5H10O2 are used? b. How many moles of H2O are produced? c. How many moles of C5H10O2 would you need to use to produce 4.42 moles of CO2 given that there is an excess of O2?How many grams of O2 are required to produce 100.0 g of SO2 ? (S=32.06, O=16) 4 FeS2 + 11 O2 ------ 2 Fe2O3 + 8 SO2 A. 36.3 g B. 49.9 g C. 68.7 g D. No correct answer given
- Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 --->5CaO + 2V In one process, 1.540×103 g of V2O5 react with 2.100×103 g Ca. (a) Calculate the theoretical yield of V. _________ g (b) Calculate the percent yield if 807.0 g of V are obtained. __________ % Report your answers to the correct number of significant figures.Adipic acid, H2C6H8O4, is used to produce nylon. It is made commercially by a controlled reaction between cyclohexane ( C6H12 ) and O2:. (Only the 4th sub part (d) is needed to be answered). 2 C6H12 (l) + 5 O2 (g) → 2 H2C6H8O4 (l) + 2 H2O (g) (Given: Atomic Wts (g/mol): C= 12.01 ; H=1.01 ; O=16.00 ) If 25.0 g of cyclohexane is reacted with 20.0 g of O2, a. Identify the limiting reactant and excess reactant? b. How much in grams of the excess reactant will be left after the reaction? c. What is the theoretical yield in terms of the product adipic acid? d. If the actual yield is 33.5 g, what is the % yield of adipic acid?Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 longrightarrow 5CaO + 2V In one process, 1.540 × 103 g of V2O5 react with 2.120 × 103 g Ca. (a) Calculate the theoretical yield of V. g (b) Calculate the percent yield if 807.0 g of V are obtained. % Report your answers to the correct number of significant figures.
- Please answer thank you 1. Methanol (CH3OH), is an excellent fuel and can be made by the reaction of CO and H2. CO + 2H2 ––> CH3OH Suppose 356 g of CO are mixed with 65 g of H2. a) What is the Limiting Reagent b) What is the maximum amount of CH3OH that can be formed? c.) What mass of the Excessive Reagent is reacted.? What mass is unreacted? c.) If 380 g of CH3OH is actually obtained , how much is the percentage yield.For the reaction C4H10 + O2 --> CO2 + H2O a) what weight of C4H10 in grams is needed for 3.01 x 10E23 particles of O2? b) how many moles of CO2 will be produced from 5.0 moles of C4H10? c) what weight in grams of H2O will be produced from 12.5 ml of C4H10? density (p)?of C4H10 = 0.506 g/mL1. How many grams of O2 are required to burn 25.0 moles of C10H8? C10H8 + 12 O2 ----> 10 CO2 + 4 H2O Group of answer choices No correct answer is given 9.60 x 103 g 66.7 g 33 g 2. How many grams of O2 are required to produce 100. g of SO2? 4 FeS2 + 11 O2 ----> 2 Fe2O3 + 8 SO2 Group of answer choices 36.3 g 68.7 g No correct answer is given 49.9 g 3. Consider the following reaction: 2 Na + 2 H2O -----> 2 NaOH + H2 When 200. g of Na were reacted, 7.32 g of H2 were collected. The percent yield was Group of answer choices No correct answer is given 78.0% 100. % 50.0%