CO2(g)+ 2 H2Og)CH4g) + 2 02(g)What mass of water is produced by the complete reaction of 10. g of methane?5.7 g23 g18 gO 11 g

Given the balanced reaction, CH4(g) + 2O2(g) → CO2(g) + 2 H2O(g) mass of methane = 10. g

Answered: CH4(g) + 2 O2ie) CO2(g) + 2 H2O(g) What…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.120QE

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The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)
Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.
The reaction of methane and water is one way to prepare hydrogen for use as a fuel: CH4(g) + H2O(g) CO(g) + 3 H2(g) If you begin with 995 g of CH4 and 2510 g of water, (a) Which reactant is the limiting reactant? (b) What is the maximum mass of H2 that can be prepared? (c) What mass of the excess reactant remains when the reaction is completed?
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.
Quicklime, CaO, is formed when calcium hydroxide is heated. Ca(OH)2(s) → CaO(s) + H2O(ℓ) The theoretical yield is 65.5 g but only 36.7 g quicklime I is produced. Calculate the percent yield.
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?

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CH4(g) + 2 O2ie) CO2(g) + 2 H2O(g) What mass of water is produced by the complete reaction of 10. g of methane? O 5.7 g O 23 g O 18 g O 11 g