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- In 1997, at the United Nations Conference on Climate Change, the major industrial nations agreed to expand their re-search efforts to develop renewable sources of carbon-basedfuels. For more than a decade, Brazil has been engaged in aprogram to replace gasoline with ethanol derived from the rootcrop manioc (cassava).(a) Write separate balanced equations for the complete combus-tion of ethanol (C₂H₅OH) and of gasoline (represented by theformula C₈H₁₈).(b) What mass of oxygen is required to burn completely 1.00 Lof a mixture that is 90.0% gasoline (d=0.742 g/mL) and 10.0%ethanol (d=0.789 g/mL) by volume?(c) If 1.00 mol of O₂ occupies 22.4 L, what volume of O₂ isneeded to burn 1.00 L of the mixture?(d) Air is 20.9% O₂ by volume. What volume of air is needed toburn 1.00 L of the mixture?3. Based on the reactions: 1. 2H,S) + 302 (g)→2SO2 (g) + 2H;O AH1 =- 1035.94 kJ 2. 2SO3 (2) →2S02 (2) + O2 (g) AH2 =+197.78 kJ 3. 2H,Sg) + O2 (g)→2S¾) + 2H;O[g) AH3 = +110.02 kJ Use Hess's law to calculate H for: 2S(5) + 302 (2)→2SO3 (g)(1) Write the structual formulas for the 5 isomers of C6H14 (2) Complete the following equations for reactions of hydrocarbons. (a) C4H10 + 02 (B) CH3-CH=CH2 + KMnO4 + H2O ---------- (don't balance) (c) CH3- CH=CH2 + Br2 -----------
- Assume that combustion of C6H8O6 is a complete reaction. So, which of the followings show the correct balanced reaction?A) C6H8O6 +4O(g) ---> 6 CO(g) + 4 H2O(s)B) C6H8O6 + 10 O(g)----> 6CO2(g) + 4H2O(s)C) C6H8O6+ 5 O2(g) ---->6CO2(g) + 4 H2O(s)D) C6H8O6+ 8 O2(g) ---->6CO2(g) + 4 H2O(s)E) C6H8O6+ 2 O2(g) ---->6CO(g) + 4 H2O(s)9,Which of the following is a combustion reaction? Group of answer choices A, H2SO4(aq) + Na2CO3(aq) =>Na2SO4(aq) + H2O(l)+ CO2(g) B, Ca(s) + 2HCl(aq) => CaCl2(aq) + H2(g) C, C2H4(g) + 3O2(g) => 2H2O(l)+ 2CO2(g) D, H2SO4(aq) + 2NaOH(aq) =>Na2SO4(aq) + 2H2O(l) E, Mg(s) +Cl2(aq) =>MgCl2(s) F, 2NaOH(aq) + MgCl2(aq)=> 2 NaCl(aq) + Mg(OH)2(s)1. Given the equation for the combustion of isopropyl alcohol 2 C3H7OH +9 02 6 CO2 +8 H2O Set up the mole ratio of (a) CO2 to C3H7OH (b) C3H7OH to 02 (c) O2 to CO2 (d) H2O to C3H7OH (e) CO2 to H2O (f) H2O to O2
- Aspirin, C6H4 (CO2H) (CO2CH3), can be prepared in the chemistry laboratory by the reaction of salicylic acid, C6H4 (CC2H) (OH), with acetic anhydride, (CH3CO)2O 2C6H4(CO2H)(OH)+(CH3CO)2O>>C6H4(CO2H)(CO2CH3)+H2O What volume of acetic anhydride (density, 1.0820 g/cm3) is required to produce 1.00 kg of aspirin, assuming a 100% yield?Write a balanced chemical equation for the reaction that occurswhen (a) titanium metal reacts with O2(g); (b) silver(I)oxide decomposes into silver metal and oxygen gas whenheated; (c) propanol, C3H7OH(l) burns in air; (d) methyltert-butyl ether, C5H12O(l), burns in air.1-butanol yields 1-bromobutane in the presence of concentrated sulfuric acid and an excess of sodium bromide. CH3CH2CH2CH2OH (1) – CH3 CH2CH,CH2B (I) If 17.12 ml of 1-butanol produced 14.77 g of 1-bromobutane, the percentage yield of the product equals: (Assume the density of 1-butanol is 0.81 g/mL, the molar mass of 1-butanol is 74 g/mol, and the molar mass of 1-bromobutane is 137 g/mol.) %
- The complete combustion of 0.32 moles of propane, C3H8, wil C3H8(g) + 5 02(g) --> 3 CO2(g) + 4 H2O(g)Incomplete combustion: _CH4(g) + _O2(g) —> _C(s) + _H2O(g).1. Write the combustion equations for (a) Complete combustion in theoretical air of 1 mol of gasoline, butane C4 H10 (b) Combustion with 21% excess air (c) Combustion with 9% CO in the product 2. Determine the (d) theoretical air-fuel ratio (e) Actual air-fuel ratio