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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

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.* [Input Field: _____________ g NH₃] Submit --- **Part C** How many grams of H₂ are needed to produce 10.59 g of NH₃? *Express your answer numerically in grams.* [Input Field: _____________ g H₂] Submit
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.* [Input Field: _____________ g NH₃] Submit --- **Part C** How many grams of H₂ are needed to produce 10.59 g of NH₃? *Express your answer numerically in grams.* [Input Field: _____________ g H₂] Submit
**Educational Content on Stoichiometry** **Learning Goal:** Understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. **Stoichiometry** is the study of the quantitative relationships among reactants and products in a balanced chemical reaction. It allows for the conversion of mass, number of moles, or number of particles between products and reactants, using mole ratios as shown in the flowchart below: **Flowchart Explanation:** 1. **Substance A:** - Convert the number of particles to moles using Avogadro's number. - Convert moles to mass using the molar mass. - Use the coefficients from the balanced chemical equation to convert moles of Substance A to moles of Substance B. 2. **Substance B:** - Convert moles to the number of particles using Avogadro's number. - Convert moles to mass using the molar mass. **Converting between Quantities:** To convert from a given quantity of one reactant or product to the quantity of another: - Convert the given quantity to moles. Use molar masses to convert masses to moles, and Avogadro's number (6.02 x 10²³ particles per mol) to convert the number of particles to moles. - Convert moles of the given reactant or product to moles of the desired one, using the coefficients from the balanced chemical equation. - Convert moles of the desired reactant or product back into the desired units (mass or number of particles). **Example Reaction:** For the chemical equation \(2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}\): - The coefficients indicate that 2 mol of \(\text{H}_2\) reacts with 1 mol of \(\text{O}_2\) to produce 2 mol of \(\text{H}_2\text{O}\). **Reaction of Hydrogen and Nitrogen to Form Ammonia:** Hydrogen gas (\(\text{H}_2\)) reacts with nitrogen gas (\(\text{N}_2\)) to form ammonia gas (\(\text{NH}_3\)), according to the equation: \[ 3\text{H}_2(g) + \text{N}_2(g) \rightarrow 2\text{NH}_
Transcribed Image Text:**Educational Content on Stoichiometry** **Learning Goal:** Understand how to use stoichiometry to convert between quantities of reactants and products in chemical equations. **Stoichiometry** is the study of the quantitative relationships among reactants and products in a balanced chemical reaction. It allows for the conversion of mass, number of moles, or number of particles between products and reactants, using mole ratios as shown in the flowchart below: **Flowchart Explanation:** 1. **Substance A:** - Convert the number of particles to moles using Avogadro's number. - Convert moles to mass using the molar mass. - Use the coefficients from the balanced chemical equation to convert moles of Substance A to moles of Substance B. 2. **Substance B:** - Convert moles to the number of particles using Avogadro's number. - Convert moles to mass using the molar mass. **Converting between Quantities:** To convert from a given quantity of one reactant or product to the quantity of another: - Convert the given quantity to moles. Use molar masses to convert masses to moles, and Avogadro's number (6.02 x 10²³ particles per mol) to convert the number of particles to moles. - Convert moles of the given reactant or product to moles of the desired one, using the coefficients from the balanced chemical equation. - Convert moles of the desired reactant or product back into the desired units (mass or number of particles). **Example Reaction:** For the chemical equation \(2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}\): - The coefficients indicate that 2 mol of \(\text{H}_2\) reacts with 1 mol of \(\text{O}_2\) to produce 2 mol of \(\text{H}_2\text{O}\). **Reaction of Hydrogen and Nitrogen to Form Ammonia:** Hydrogen gas (\(\text{H}_2\)) reacts with nitrogen gas (\(\text{N}_2\)) to form ammonia gas (\(\text{NH}_3\)), according to the equation: \[ 3\text{H}_2(g) + \text{N}_2(g) \rightarrow 2\text{NH}_
Expert Solution
Step 1: Introduction

To solve this problem, we have to use the given balanced chemical equation. 

Given balanced chemical equation is 

3H2(g)  ----> 2NH3 (g) 



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