lon. For the following reaction, 5.79 grams of propane (C3Hg) are allowed to react with 24.3 grams of oxygen gas. propane (C3H8)(g) + oxygen (g) → carbon dioxide(g) + water (g) What is the maximum amount of carbon dioxide that can be formed? Mass= g What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? Mass= g

lon. For the following reaction, 5.79 grams of propane (C3Hg) are allowed to react with 24.3 grams of oxygen gas. propane (C3H8)(g) + oxygen (g) → carbon dioxide(g) + water (g) What is the maximum amount of carbon dioxide that can be formed? Mass= g What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? Mass= g

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem 20STP

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Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. l type='a'> Write the balanced equation for the reaction that is (occurring. including all phases. If a 100.0-g sample of calcium carbide (CaC2)is initially reacted with 50.0 g of water, which reactant is limiting? Prove that mass is conserved for the reactant amounts used in pan b.
Consider the following reaction: 4NH3(g)4NO(g)+6H2O(g) If a container were to have 10 molecules of O2 and 10 molecules of NH3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?
Alkali metal hydroxides are sometimes used to “scrub” excess carbon dioxide from the air in closed spaces (such as submarines and spacecraft). For example, lithium hydroxide reacts with carbon dioxide according to the unbalanced chemical equation :math>LiOH(s)+CO2(g)Li2CO3(s)+H2O(g) ppose a lithium hydroxide canister contains 155 g of LiOH(s). What mass of CO2(g)will the canister be able to absorb? If it is found that after 24 hours of use the canister has absorbed 102 g of carbon dioxide, what percentage of its capacity has been reached?
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): :math>C5H12(l)+O2(g)CO2(g)+H2O(l) a 20.4-gram sample of pentane is burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is given below: SO2(g)+NaOH(s)Na2SO3(s)+H2O(l) Assuming you react 38.3 g sulfur dioxide with 32.8 g sodium hydroxide and assuming that the reaction goes to completion, calculate the mass of each product formed.
If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: :math>2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) lculate the mass of sodium carbonate that will remain if a 1.52-g sample of sodium hydrogen carbonate is heated.
In a blast furnace at high temperature, iron(III) oxide in ore reacts with carbon monoxide to produce metallic iron and carbon dioxide. The liquid iron produced is cooled and weighed. The reaction is run repeatedly with the same initial mass of iron(III) oxide, 19.0 g, but differing initial masses of carbon monoxide. The masses of iron obtained arc shown in this graph. (a) Write the balanced chemical equation for this reaction. (b) Calculate the mass of CO required to react completely with 19.0 g iron(III) oxide. (c) Calculate the mass of carbon dioxide produced when the reaction converts 10.0 g iron(III) oxide completely to products. (d) From the graph, determine which reactant is limiting when less than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (e) From the graph, determine which reactant is limiting when more than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (f) Calculate the percent yield if 24.0 g iron(III) oxide reacted with 20.0 g carbon monoxide to produce 15.9 g metallic iron. (g) Calculate the minimum mass of additional limiting reactant required to react with all of the excess of nonlimiting reactant from part (f).
he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
Nitrogen and oxygen react as follows: N2(g)+2O2(g)2NO2(g) Suppose 1.25mol of N2 and 50.0g of O2 are mixed together. a.Which one is the limiting reactant? b.What is the maximum mass in grams of NO2 that can be produced from the mixture?