Methanol, CH3OH, is an important industrial compound that is produced from the following (unbalanced) reaction. CO(g) + H2(g) CH3OH(g) What mass of...

Methanol, CH3OH, is an important industrial compound that is produced from the following (unbalanced) reaction.CO(g) + H2(g) CH3OH(g)What mass of each reactant would be needed to produce 100.0 kg of methanol?COg H2g6. –/2 points Notes Question: HoltMChem06 9.P.010.Nitrogen combines with oxygen in the atmosphere during lightning flashes to form nitrogen monoxide, NO, which then reacts further with O2 to produce nitrogen dioxide, NO2.(a) What mass of NO2 is formed when NO reacts with 376 g O2?g(b) How many grams of NO are required to react with this amount of O2?g7. –/3 points Notes Question: HoltMChem06 9.P.011.As early as 1938, the use of NaOH was suggested as a means of removing CO2 from the cabin of a spacecraft according to the following (unbalanced) reaction.NaOH + CO2 Na2CO3 + H2O(a) If the average human body discharges 915.0 g CO2 per day, how many moles of NaOH are needed each day for each person in the spacecraft?mol(b) How many moles of each product are formed?Na2CO3molH2Omol8. –/2 points Notes Question: HoltMChem06 9.P.012.The double-replacement reaction between silver nitrate and sodium bromide produces silver bromide, a component of photographic film.(a) If 7.50 mol of silver nitrate react, what mass of sodium bromide is required?g(b) What mass of silver bromide is formed?g9. –/4 points Notes Question: HoltMChem06 9.P.013.In a soda-acid fire extinguisher, concentrated sulfuric acid reacts with sodium hydrogen carbonate to produce carbon dioxide, sodium sulfate, and water.(a) How many moles of sodium hydrogen carbonate would be needed to react with 196.0 g of sulfuric acid?mol(b) How many moles of each product would be formed?carbon dioxidemolsodium sulfatemolwatermol10. –/7 points Notes Question: HoltMChem06 9.P.014.Sulfuric acid reacts with sodium hydroxide according to the following equation.H2SO4 + NaOH Na2SO4 + H2O(a) Balance the equation for this reaction. (Use the lowest possible coefficients.) Na2SO4 + H2O (b) What mass of H2SO4 would be required to react with 0.79 mol NaOH? g (c) What mass of each product is formed by this reaction? Na2SO4 g H2O g11. –/3 points Notes Question: HoltMChem06 9.P.015.Copper reacts with silver nitrate through single replacement.(a) If 2.55 g of silver are produced from the reaction, how many moles of copper(II) nitrate are also produced?mol (b) How many moles of each reactant are required in this reaction? coppermolsilver nitratemol12. –/3 points Notes Question: HoltMChem06 9.P.016.Aspirin, C9H8O4, is produced through the following reaction of salicylic acid, C7H6O3, and acetic anhydride, C4H6O3.C7H6O3(s) + C4H6O3(l) C9H8O4(s) + HC2H3O2(l)(a) What mass of aspirin (kg) could be produced from 79.4 mol of salicylic acid? kg(b) What mass of acetic anhydride (kg) would be required? kg(c) At 20°C, how many liters of acetic acid, HC2H3O2, would be formed? The density of HC2H3O2 is 1.05 g/mL.L13. –/3 points Notes Question: HoltMChem06 9.P.022.Given the reactant amounts specified in each chemical equation, determine the limiting reactant in each case.(a) HCl + NaOH NaCl + H2O 1.2 mol HCl and 3.7 mol NaOHHCl(b) Zn + 2 HCl ZnCl2 + H2 3.7 mol Zn and 4.8 mol HClZn(c) 2 Fe(OH)3 + 3 H2SO4 Fe2(SO4)3 + 6 H2O 6.0 mol Fe(OH)3 and 6.3 mol H2SO4Fe(OH)314. –/3 points Notes Question: HoltMChem06 9.P.023.Given the reactant amounts specified in each chemical equation, determine the amount in moles of excess reactant that remains.(a) HCl + NaOH NaCl + H2O 2.2 mol HCl and 3.7 mol NaOH amount of excess reactant mol (b) Zn + 2 HCl ZnCl2 + H2 3.7 mol Zn and 6.0 mol HCl amount of excess reactant mol (c) 2 Fe(OH)3 + 3 H2SO4 Fe2(SO4)3 + 6 H2O 6.4 mol Fe(OH)3 and 5.9 mol H2SO4 amount of excess reactant mol15. –/6 points Notes Question: HoltMChem06 9.P.024.Given the reactant amounts specified in each chemical equation, calculate the amount in moles of each product formed.(a) HCl + NaOH NaCl + H2O 2.4 mol HCl and 2.3 mol NaOH NaCl mol H2O mol (b) Zn + 2 HCl ZnCl2 + H2 4.1 mol Zn and 6.0 mol HCl ZnCl2 mol H2 mol (c) 2 Fe(OH)3 + 3 H2SO4 Fe2(SO4)3 + 6 H2O 5.6 mol Fe(OH)3 and 6.7 mol H2SO4 Fe2(SO4)3 mol H2O mol16. –/6 points Notes Question: HoltMChem06 9.P.025.(a) If 3.70 mol of copper and 6.80 mol of silver nitrate are available to react by single replacement, identify the limiting reactant.copper(b) Determine the amount in moles of excess reactant remaining. mol (c) Determine the amount in moles of each product formed. silver mol copper(II) nitrate mol (d) Determine the mass of each product formed. silver g copper(II) nitrate g17. –/4 points Notes Question: HoltMChem06 9.P.026.Sulfuric acid reacts with aluminum hydroxide by double replacement.(a) If 47.0 g of sulfuric acid react with 36.0 g of aluminum hydroxide, identify the limiting reactant.sulfuric acid(b) Determine the mass of excess reactant remaining. g (c) Determine the mass of each product formed. Assume 100% yield. aluminum sulfate g water g18. –/4 points Notes Question: HoltMChem06 9.P.028.Calculate the indicated quantity for each of the various chemical reactions given.(a) theoretical yield = 17.4 g, actual yield = 15.1 g, percentage yield = ? % (b) theoretical yield = 1.2 g, percentage yield = 94.0%, actual yield = ?g (c) theoretical yield = 5.05 g, actual yield = 4.58 g, percentage yield = ? % (d) theoretical yield = 2.75 g, percentage yield = 44.0%, actual yield = ?g19. –/1 points Notes Question: HoltMChem06 9.P.029.The percentage yield for the following reaction is 81.4%.PCl3 + Cl2 PCl5What mass of PCl5 is expected from the reaction of 85.7 g PCl3 with excess chlorine?g20. –/1 points Notes Question: HoltMChem06 9.P.030.The Ostwald process for producing nitric acid from ammonia consists of the following steps.4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) 2 NO(g) + O2(g) 2 NO2(g) 3 NO2(g) + H2O(g) 2 HNO3(aq) + NO(g) If the yield in each step is 93.5%, how many grams of nitric acid can be produced from 5.30 kg of ammonia? g21. –/1 points Notes Question: HoltMChem06 9.P.031.Magnesium is obtained from sea water. Ca(OH)2 is added to sea water to precipitate Mg(OH)2. The precipitate is filtered and reacted with HCl to produce MgCl2. The MgCl2 is electrolyzed to produce Mg and Cl2. If 210.0 g of magnesium are recovered from 1290. g MgCl2, what is the percentage yield for this reaction? %22. –/1 points Notes Question: HoltMChem06 9.P.032.Phosphate baking powder is a mixture of starch, sodium hydrogen carbonate, and calcium dihydrogen phosphate. When mixed with water, phosphate baking powder releases carbon dioxide gas, causing a dough or batter to bubble and rise.2 NaHCO3(aq) + Ca(H2PO4)2(aq) Na2HPO4(aq) + CaHPO4(aq) + 2 CO2(g) + 2 H2O(l)If 0.900 L CO2 is needed for a cake and each kilogram of baking powder contains 168 g of NaHCO3, how many grams of baking powder must be used to generate this amount of CO2? The density of CO2 at baking temperature is about 1.20 g/L.g23. –/1 points Notes Question: HoltMChem06 9.P.033.Coal gasification is a process that converts coal into methane gas. If this reaction has a percentage yield of 92.0%, what mass of methane can be obtained from 1070 g of carbon?2 C(s) + 2 H2O(l) CH4(g) + CO2(g)g24. –/2 points Notes Question: HoltMChem06 9.P.041.The steel-making process described in the Transition Metal section of the Elements Handbook shows the equation for the formation of iron carbide. Use this equation (given below) to answer the following questions.3 Fe + C Fe3C(a) If 3.93 103 kg of iron is used in a steel-making process, what is the minimum mass of carbon needed to react with all of the iron?kg (b) What is the theoretical mass of iron carbide that is formed?kg25. –/3 points Notes Question: HoltMChem06 9.P.043.The reactions of oxide compounds to produce carbonates, phosphates, and sulfates are described in the section on oxides in Group 16 of the Elements Handbook. Use those equations (given below) to answer the following questions.MgO(s) + CO2(g) MgCO3(s) 6 CaO(s) + P4O10(s) 2 Ca3(PO4)2(s) CaO(s) + SO3(g) CaSO4(s)(a) What mass of CO2 is needed to react with 176.6 g MgO? g (b) What mass of magnesium carbonate is produced? g (c) When 45.5 g P4O10 is reacted with an excess of calcium oxide, what mass of calcium phosphate is produced? g