Concept explainers
Interpretation:
The limiting reactant when
Concept introduction:
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Introductory Chemistry: Concepts and Critical Thinking (8th Edition)
- Electrolysis Determine the theoretical and percent yield of hydrogen gas if 36.0 g ofwater undergoes electrolysis to produce hydrogen and oxygen and 3.80 g of hydrogen is collected.arrow_forwardThe simplest example of the hydrogenation of a carbon-carbon double bond is the reaction between ethene and hydrogen in the presence of nickel: CH2=CH2+H2NiCH3CH3. When 5.20g of ethene react with excess hydrogen gas, the reaction yields 4.75g of ethane. What is the percentage yield for this reaction?arrow_forwardNitrogen 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?arrow_forward
- Small quantities of ammonia gas can be generated in the laboratory by heating an ammonium salt with a strong base. For example, ammonium chloride reacts with sodium hydroxide according to the following balanced equation: :math>NH4Cl(s)+NaOH(s)NH3(g)+NaCl(s)+N2O(g) at mass of ammonia gas is produced if 1.39 g of ammonium chloride reacts completely?arrow_forwardAlkali 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?arrow_forwardConsider the following balanced chemical equation: A+5B3C+4D a. Equal masses of A and B are reacted. Complete each of the following with either A is the limiting reactant because ; B is the limiting reactant because ____ ; or we cannot determine the limiting reactant because _____ i. If the molar mass of A is greater than the molar mass of B, then ii. If the molar mass of B is greater than the molar mass of A, then b. The products of the reaction are carbon dioxide (C) and water (D). Compound A has a similar molar mass to carbon dioxide. Compound B is a diatomic molecule. Identify compound B, and support your answer. c. Compound A is a hydrocarbon that is 81.7 1% carbon by mass. Determine its empirical and molecular formulas.arrow_forward
- Outline the steps needed to determine the limiting reactant when 0.50 mol of Cr and 0.75 mol of H3PO4 react according to the following chemical equation. 2Cr+2H3PO42CrPO4+3H2 Determine the limiting reactant.arrow_forwardConsider a reaction represented by the following balanced equation :math>2A+3BC+4D u find that it requires equal masses of A and B so that there are no reactants left over. Which of the following is true? Justify your choice. l type='a'> The molar mass of A must be greater than the molar mass of B. i>The molar mass of A must be less than the molar mass of B. i>The molar mass of A must be the same as the molar mass of B.arrow_forwardWhen elemental boron, B, is burned in oxygen gas, the product is diboron trioxide. If the diboron trioxide is then reacted with a measured quantity of water, it reacts with the water to form what is commonly known as boric acid, B(OH)3 . Write a balanced chemical equation for each of these processes.arrow_forward
- Elemental phosphorus can be prepared from calciumphosphate via the overall reaction 2Ca3( PO4)2+6SiO2+10C6CaSiO3+P4+10CO Calculate the minimum mass of Ca3( PO4)2 required toproduce 69.8gP4 . What mass of CaSiO3 is generated as aby-product?arrow_forwardThe first step in the Ostwald process for manufacturing nitric acid is the reaction between ammonia and oxygen described by the equation 4NH3+5O24NO+6H2O. Use this equation to answer all parts of this question. a How many moles of ammonia will react with 95.3 moles of oxygen? b How many moles of nitrogen monoxide will result from the reaction of 2.89 moles of ammonia? c If 3.35 moles of water is produced, how many moles of nitrogen monoxide will also be produced?arrow_forwardonsider the balanced chemical equation :math>4Al(s)+3O2(g)2Al2O3(s). at mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely?arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning