18 **Text from Image:**According to the following reaction, how many moles of **iron(II) oxide** will be formed upon the complete reaction of **23.0 grams** of iron with excess **oxygen gas**?\[ \text{iron (s) + oxygen (g) } \rightarrow \text{iron(II) oxide (s)} \]\[ \text{[ \_\_\_\_\_ moles iron(II) oxide ]} \]**Explanation:**The given chemical equation involves the reaction between solid iron (\( \text{Fe} \)) and gaseous oxygen (\( \text{O}_2 \)) to produce solid iron(II) oxide (\( \text{FeO} \)). The task is to calculate how many moles of iron(II) oxide will be produced when 23.0 grams of iron completely reacts with an excess of oxygen gas. A blank is provided for the student to fill in the number of moles of iron(II) oxide formed.

Given that: Mass of iron = 23.0 g Molar mass of iron = 55.8g/mol

According to the following reaction, how many moles of iron(II) oxide will be formed upon the complete reaction of 23.0 grams of iron with excess oxygen gas? iron (s) + oxygen (g) →iron(II) oxide (s) moles iron(II) oxide

According to the following reaction, how many moles of iron(II) oxide will be formed upon the complete reaction of 23.0 grams of iron with excess oxygen gas? iron (s) + oxygen (g) →iron(II) oxide (s) moles iron(II) oxide

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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