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▼ Part B How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂. Express your answer numerically in grams. ► View Available Hint(s) VE ΑΣΦ Submit Part C VE ΑΣΦ ? How many grams of H₂ are needed to produce 10.59 g of NH3? Express your answer numerically in grams. ► View Available Hint(s) Submit g NH3 ? g H₂

▼ Part B How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂. Express your answer numerically in grams. ► View Available Hint(s) VE ΑΣΦ Submit Part C VE ΑΣΦ ? How many grams of H₂ are needed to produce 10.59 g of NH3? Express your answer numerically in grams. ► View Available Hint(s) Submit g NH3 ? g H₂

Introductory Chemistry: An Active Learning Approach
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Mark S. Cracolice, Ed Peters
Chapter10: Quantity Relationships In Chemical Reactions
Section: Chapter Questions
Problem 70E: Classify each of the following statements as true or false: a Coefficients in a chemical equation...
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Answer part A,B, and C
▼ Part B How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂. Express your answer numerically in grams. View Available Hint(s) VE ΑΣΦ Submit Part C How many grams of H₂ are needed to produce 10.59 g of NH3? Express your answer numerically in grams. ► View Available Hint(s) 5 ΑΣΦ g NH3 Submit g H₂
Transcribed Image Text:▼ Part B How many grams of NH3 can be produced from 4.86 mol of N₂ and excess H₂. Express your answer numerically in grams. View Available Hint(s) VE ΑΣΦ Submit Part C How many grams of H₂ are needed to produce 10.59 g of NH3? Express your answer numerically in grams. ► View Available Hint(s) 5 ΑΣΦ g NH3 Submit g H₂
Learning Goal: To understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. Stoichiometry describes the quantitative relationships among the reactants and products of a balanced reaction by directly comparing mole ratios. Stoichiometry can be used to convert mass, number of moles, or number of particles between products and reactants, as shown in the flowchart displayed in the figure. Substance A Substance B number of particles Avogadro's number Avogadro's number number of particles I I mass moles coefficients from balanced chemical equation moles mass I molar mass molar mass Converting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product: Review | Constants I Periodic Table . First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02 x 1023 particles per mole) to convert number of particles to moles. • Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation 2H2 + O2 2H₂O the coefficients tell us that 2 mol of H₂ reacts with 1 mol of O₂ to produce 2 mol of H₂O. ▼ • Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2, reacts with nitrogen gas, N₂, to form ammonia gas, NH3, according to the equation 3H2(g) + N2(g) →→2NH3(g) NOTE: Throughout this tutorial use molar masses expressed to five significant figures. Part A How many moles of NH3 can be produced from 15.0 mol of H₂ and excess N₂? Express your answer numerically in moles. ►View Available Hint(s) |VLI ΑΣΦ 4 ? mol NH3
Transcribed Image Text:Learning Goal: To understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. Stoichiometry describes the quantitative relationships among the reactants and products of a balanced reaction by directly comparing mole ratios. Stoichiometry can be used to convert mass, number of moles, or number of particles between products and reactants, as shown in the flowchart displayed in the figure. Substance A Substance B number of particles Avogadro's number Avogadro's number number of particles I I mass moles coefficients from balanced chemical equation moles mass I molar mass molar mass Converting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product: Review | Constants I Periodic Table . First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02 x 1023 particles per mole) to convert number of particles to moles. • Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation 2H2 + O2 2H₂O the coefficients tell us that 2 mol of H₂ reacts with 1 mol of O₂ to produce 2 mol of H₂O. ▼ • Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2, reacts with nitrogen gas, N₂, to form ammonia gas, NH3, according to the equation 3H2(g) + N2(g) →→2NH3(g) NOTE: Throughout this tutorial use molar masses expressed to five significant figures. Part A How many moles of NH3 can be produced from 15.0 mol of H₂ and excess N₂? Express your answer numerically in moles. ►View Available Hint(s) |VLI ΑΣΦ 4 ? mol NH3
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