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- ATOM ECONOMY: Ethylene oxide, C2H4O, is an important industrial chemical [as it isthe starting place to make such important chemicals as ethylene glycol (antifreeze)and various polymers]. One way to make the compound is called the “chlorohydrinroute.”C2H4 + Cl2 + Ca(OH)2 → C2H4O + CaCl2 + H2OAnother route is the modern catalytic reaction.C2H4 + 1/2 O2 → C2H4O(a) Calculate the % atom economy for the production of C2H4O in each of thesereactions. Which is the more efficient method?(b) What is the percent yield of C2H4O if 867 g of C2H4is used to synthesize 762 gof the product by the catalytic reaction?Dilute sulfuric acid can be used to remove rust iron (III) oxide from iron in a process known as pickling. a) Write the equation for the reaction between iron (III) oxide and b) calculate the mass of rust which can be removed by reaction with 49g of sulphuric acid. a) 3H2SO4 + Fe2O3 = Fe2(SO4)3 + 3H2O note: I've done part a but I need help with part b. This is a question from O level December 2000 past papers.2CO (g) + O2 (g) ⟶ 2 CO2 (g) Which of the following choices best describes the ΔS in the above equation?
- When magnesium metal is burned in air (Figure 3.6), twoproducts are produced. One is magnesium oxide, MgO. Theother is the product of the reaction of Mg with molecularnitrogen, magnesium nitride. When water is added to magnesiumnitride, it reacts to form magnesium oxide and ammoniagas. (a) Based on the charge of the nitride ion (Table2.5), predict the formula of magnesium nitride. (b) Write abalanced equation for the reaction of magnesium nitridewith water. What is the driving force for this reaction? (c) Inan experiment, a piece of magnesium ribbon is burned in airin a crucible. The mass of the mixture of MgO and magnesiumnitride after burning is 0.470 g. Water is added to thecrucible, further reaction occurs, and the crucible is heated todryness until the final product is 0.486 g of MgO. What wasthe mass percentage of magnesium nitride in the mixture obtainedafter the initial burning? (d) Magnesium nitride canalso be formed by reaction of the metal with ammonia at hightemperature.…A chemistry student performed the reaction: SnCl4(l) + 2H2Se(g) -> SnSe2(s) + 4HCl(g) in lab. The student started with 0.34 moles of SnCl4 and 0.46 moles of H2Se. The amount of HCl(g) actually produced by the student was 0.26 moles of HCl. a. what is the limiting reagent? b. what is the % yield for this reaction?Determine the amount of carbon dioxide produced when 0.35 mol of calcium carbonate decomposes, and balance the equation first. CaCO3 (s) ------------ CaO(s) + CO2 (g). Show your work
- For the reaction C6H1206 + 02 -, H2O + CO2, how many moles of glucose (C6H1206) are required to produce 6.60 moles of carbon dioxide?The following diagram shows the combination reactionbetween hydrogen, H2, and carbon monoxide, CO, toproduce methanol, CH3OH (white spheres are H, black spheresare C, red spheres are O). The correct number of CO moleculesinvolved in this reaction is not shown. [Section 3.1](a) Determine the number of CO molecules that should beshown in the left (reactants) box.(b) Write a balanced chemical equation for the reaction.PRACTICE ANOTHER C4H10 + O2 → CO2 + H2O (unbalanced)What mass of CO2 is produced in the complete combustion of 78.8 g of butane, C4H10, to CO2 and H2O? gWhat mass of oxygen is required for the complete reaction? gWhat mass of water is produced? g
- how many moles of hydrogen gas is generated per mole of zinc that reacts with hydrochloric acid? A. 1.5 B. 1 C. 0.5 D. 2 E. 0.75 F. 2.5 G. 1.25 H. 3 F. No hydrogen gas is produced since since zinc and hydrochloric don’t react.A container holds 75.0 g of CuO and 5.00 g of H₂. The following reaction occurs: CuO + H₂ --> Cu + H₂O. If the reaction produces 45.5 g of Cu, calculate the % yield. a. 76.0% b. 29.0% c. 50.5% d. 68.1%In the reaction between CO and Fe3O4 , the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 42.9 g Fe. Calculate the percentage yield. Is this correct answer 90.9%?
