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Question 4 For the reaction Fe203(s) + 3 COg) → 2 Fe(s) + 3 CO2(g) where 39.6 grams of Fe2O3(s) reacts at 250°C, 1.2 atm: How many moles of CO2(g) are produced? [A] What Volume of CO2(g) is produced? [B]

Question 4 For the reaction Fe203(s) + 3 COg) → 2 Fe(s) + 3 CO2(g) where 39.6 grams of Fe2O3(s) reacts at 250°C, 1.2 atm: How many moles of CO2(g) are produced? [A] What Volume of CO2(g) is produced? [B]

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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**Question 4** For the reaction \( \text{Fe}_2\text{O}_3(s) + 3 \text{CO}(g) \rightarrow 2 \text{Fe}(s) + 3 \text{CO}_2(g) \) where 39.6 grams of \( \text{Fe}_2\text{O}_3(s) \) reacts at 250°C, 1.2 atm: - How many moles of \( \text{CO}_2(g) \) are produced? [A] - What volume of \( \text{CO}_2(g) \) is produced? [B]
Transcribed Image Text:**Question 4** For the reaction \( \text{Fe}_2\text{O}_3(s) + 3 \text{CO}(g) \rightarrow 2 \text{Fe}(s) + 3 \text{CO}_2(g) \) where 39.6 grams of \( \text{Fe}_2\text{O}_3(s) \) reacts at 250°C, 1.2 atm: - How many moles of \( \text{CO}_2(g) \) are produced? [A] - What volume of \( \text{CO}_2(g) \) is produced? [B]
### Question 3 A mixture of N₂ and O₂ contains 2.7 grams of O₂ and occupies 3.1 liters at 28°C, 810 mm Hg. - How many grams of N₂ are present? **[A]** - What is the mole fraction of O₂? **[B]** - What is the mole fraction of N₂? **[C]** - What is the partial pressure of O₂? **[D]** - What is the partial pressure of N₂? **[E]**
Transcribed Image Text:### Question 3 A mixture of N₂ and O₂ contains 2.7 grams of O₂ and occupies 3.1 liters at 28°C, 810 mm Hg. - How many grams of N₂ are present? **[A]** - What is the mole fraction of O₂? **[B]** - What is the mole fraction of N₂? **[C]** - What is the partial pressure of O₂? **[D]** - What is the partial pressure of N₂? **[E]**
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