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H;(g) + Iz(s) – 2HI(g) Given an initial mass of 17.8 g Hz, an excess of Iz, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction. Submit Determine the mass e) of the reactant, H,. consumed by the reaction. Submit The entire mass, 17.8 g, of the reactant H, is consumed by the reaction. Calculate the amount (mol) of H, in this mass. Molar mass = 2.02 g'mol mol

H;(g) + Iz(s) – 2HI(g) Given an initial mass of 17.8 g Hz, an excess of Iz, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction. Submit Determine the mass e) of the reactant, H,. consumed by the reaction. Submit The entire mass, 17.8 g, of the reactant H, is consumed by the reaction. Calculate the amount (mol) of H, in this mass. Molar mass = 2.02 g'mol mol

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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What is the balanced equation for this reaction (in lowest multiple integers)?

--- **H₂(g) + I₂(s) → 2HI(g)** 1. **Mass of HI Produced** Given an initial mass of 17.8 g H₂, an excess of I₂, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction. **Input:** - Enter mass in grams (g): [Input box] **Action:** - Submit [Button] 2. **Mass of H₂ Consumed** Determine the mass (g) of the reactant, H₂, consumed by the reaction. **Input:** - Enter mass in grams (g): [Input box] **Action:** - Submit [Button] 3. **Moles of H₂ Consumed** The entire mass, 17.8 g, of the reactant H₂ is consumed by the reaction. Calculate the amount (mol) of H₂ in this mass. **Molar mass = 2.02 g/mol** **Input:** - Enter amount in moles (mol): [Input box] **Action:** - Submit [Button] 4. **Moles of HI Formed** Given that 8.8294 mol H₂ was consumed, calculate the amount of HI formed. **Input:** - Enter amount in moles (mol): [Input box] **Action:** - Submit [Button] 5. **Mass of HI Formed** Complete consumption of H₂ yields 17.6587 mol of HI. Calculate the mass of this quantity of HI. **Molar mass = 127.91 g/mol** **Input:** - Enter mass in grams (g): [Input box] **Action:** - Submit [Button] --- This transcription elaborates on the chemical reaction process, guiding students through calculations involving mass and mole conversions within this specific chemical context.
Transcribed Image Text:--- **H₂(g) + I₂(s) → 2HI(g)** 1. **Mass of HI Produced** Given an initial mass of 17.8 g H₂, an excess of I₂, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction. **Input:** - Enter mass in grams (g): [Input box] **Action:** - Submit [Button] 2. **Mass of H₂ Consumed** Determine the mass (g) of the reactant, H₂, consumed by the reaction. **Input:** - Enter mass in grams (g): [Input box] **Action:** - Submit [Button] 3. **Moles of H₂ Consumed** The entire mass, 17.8 g, of the reactant H₂ is consumed by the reaction. Calculate the amount (mol) of H₂ in this mass. **Molar mass = 2.02 g/mol** **Input:** - Enter amount in moles (mol): [Input box] **Action:** - Submit [Button] 4. **Moles of HI Formed** Given that 8.8294 mol H₂ was consumed, calculate the amount of HI formed. **Input:** - Enter amount in moles (mol): [Input box] **Action:** - Submit [Button] 5. **Mass of HI Formed** Complete consumption of H₂ yields 17.6587 mol of HI. Calculate the mass of this quantity of HI. **Molar mass = 127.91 g/mol** **Input:** - Enter mass in grams (g): [Input box] **Action:** - Submit [Button] --- This transcription elaborates on the chemical reaction process, guiding students through calculations involving mass and mole conversions within this specific chemical context.
**Chemical Reaction Worksheets** **1. Balancing Chemical Equations:** - **Reaction:** \( \_\_\_ \text{MnO}_2(s) + \_\_\_ \text{Al}(s) \rightarrow \_\_\_ \text{Mn}(s) + \_\_\_ \text{Al}_2\text{O}_3(s) \) - *Enter the balanced equation in lowest multiple integers.* **2. Stoichiometry Calculations:** a. **Calculating Moles of MnO₂:** - *Question:* How many moles are present in 53.9 g of MnO₂? - *Enter moles of MnO₂:* b. **Mole Ratio Determination:** - **Reaction:** \( 3 \text{MnO}_2(s) + 4 \text{Al}(s) \rightarrow 3 \text{Mn}(s) + 2 \text{Al}_2\text{O}_3(s) \) - *Enter the mole ratio of Al to MnO₂:* c. **Reacting Moles of Al:** - *Question:* How many moles of Al are required to completely react with 0.620 mol MnO₂? - *Enter moles of Al:* d. **Mass of Al Required:** - *Question:* What is the mass of Al required? - *Enter mass of Al in grams:* e. **Formation of Iron(III) Chloride:** - **Reaction:** \( \text{Fe}(s) + \text{Cl}_2(g) \rightarrow \text{FeCl}_3(s) \) - *Question:* How many milligrams of iron(III) chloride result when 20.00 mg of iron is reacted with excess chlorine gas? - *Enter mass in mg of FeCl₃:* **3. Limiting Reagent Analysis:** a. **Amount of Acetic Acid Formed:** - *Question:* What amount of HC₂H₃O₂ can be formed from the amount of each reactant? - If all of the CH₃CHO was used up in the reaction, how many moles of HC₂H₃O₂ would be produced? - *Enter moles of HC₂
Transcribed Image Text:**Chemical Reaction Worksheets** **1. Balancing Chemical Equations:** - **Reaction:** \( \_\_\_ \text{MnO}_2(s) + \_\_\_ \text{Al}(s) \rightarrow \_\_\_ \text{Mn}(s) + \_\_\_ \text{Al}_2\text{O}_3(s) \) - *Enter the balanced equation in lowest multiple integers.* **2. Stoichiometry Calculations:** a. **Calculating Moles of MnO₂:** - *Question:* How many moles are present in 53.9 g of MnO₂? - *Enter moles of MnO₂:* b. **Mole Ratio Determination:** - **Reaction:** \( 3 \text{MnO}_2(s) + 4 \text{Al}(s) \rightarrow 3 \text{Mn}(s) + 2 \text{Al}_2\text{O}_3(s) \) - *Enter the mole ratio of Al to MnO₂:* c. **Reacting Moles of Al:** - *Question:* How many moles of Al are required to completely react with 0.620 mol MnO₂? - *Enter moles of Al:* d. **Mass of Al Required:** - *Question:* What is the mass of Al required? - *Enter mass of Al in grams:* e. **Formation of Iron(III) Chloride:** - **Reaction:** \( \text{Fe}(s) + \text{Cl}_2(g) \rightarrow \text{FeCl}_3(s) \) - *Question:* How many milligrams of iron(III) chloride result when 20.00 mg of iron is reacted with excess chlorine gas? - *Enter mass in mg of FeCl₃:* **3. Limiting Reagent Analysis:** a. **Amount of Acetic Acid Formed:** - *Question:* What amount of HC₂H₃O₂ can be formed from the amount of each reactant? - If all of the CH₃CHO was used up in the reaction, how many moles of HC₂H₃O₂ would be produced? - *Enter moles of HC₂
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