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Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 82.3%, how many grams of product were formed? mass of product formed: How many grams of the excess reactant remain? mass of excess reactant: 50 g g

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 82.3%, how many grams of product were formed? mass of product formed: How many grams of the excess reactant remain? mass of excess reactant: 50 g g

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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Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. **Equation:** \[ \text{equation}: \] [Text box for input] **What is the limiting reactant?** - [ ] magnesium - [ ] oxygen **If the percent yield for the reaction is 82.3%, how many grams of product were formed?** \[ \text{mass of product formed:} \] [Text box for input] g **How many grams of the excess reactant remain?** \[ \text{mass of excess reactant:} \] [Text box for input] g
Transcribed Image Text:Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.71 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. **Equation:** \[ \text{equation}: \] [Text box for input] **What is the limiting reactant?** - [ ] magnesium - [ ] oxygen **If the percent yield for the reaction is 82.3%, how many grams of product were formed?** \[ \text{mass of product formed:} \] [Text box for input] g **How many grams of the excess reactant remain?** \[ \text{mass of excess reactant:} \] [Text box for input] g
Expert Solution
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Given data :

Mass of magnesium ribbon = 3.51 g

Mass of oxygen = 8.71 g

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The excess reactant doesn't appear to be correct. Is there another answer?

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