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 net ionic equation for the reactions of Ca(s) + H2O and Mg(s) + H2O(l)?
![**Title: Writing Chemical Equations for Metal-Water Reactions**
In this section, we explore the reactions between metals and water. Below are examples of how to write equations for these reactions.
**Example Equations:**
1. **Calcium Reaction with Water:**
\[
\text{Ca(s) + 2H}_2\text{O(l) } \rightarrow \text{ Ca(OH)}_2\text{(aq) + H}_2\text{(g)}
\]
*Explanation:* Calcium metal reacts with water to form calcium hydroxide and hydrogen gas. The solid state is indicated by (s), the liquid state by (l), the aqueous state by (aq), and the gaseous state by (g).
2. **Magnesium Reaction with Water:**
\[
\text{Mg(s) + 2H}_2\text{O(l) } \rightarrow \text{ Mg(OH)}_2\text{(aq) + H}_2\text{(g)}
\]
*Explanation:* Magnesium reacts with water more slowly compared to calcium, resulting in the formation of magnesium hydroxide and hydrogen gas.
Explore these reactions further to understand the dynamics and products involved when metals are introduced to water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5014d6a8-882c-467c-b1c9-5ade3eaa5554%2Fb52578a4-a06d-4f0d-8bac-5095ff4e8eb3%2Fe54q3.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Writing Chemical Equations for Metal-Water Reactions**
In this section, we explore the reactions between metals and water. Below are examples of how to write equations for these reactions.
**Example Equations:**
1. **Calcium Reaction with Water:**
\[
\text{Ca(s) + 2H}_2\text{O(l) } \rightarrow \text{ Ca(OH)}_2\text{(aq) + H}_2\text{(g)}
\]
*Explanation:* Calcium metal reacts with water to form calcium hydroxide and hydrogen gas. The solid state is indicated by (s), the liquid state by (l), the aqueous state by (aq), and the gaseous state by (g).
2. **Magnesium Reaction with Water:**
\[
\text{Mg(s) + 2H}_2\text{O(l) } \rightarrow \text{ Mg(OH)}_2\text{(aq) + H}_2\text{(g)}
\]
*Explanation:* Magnesium reacts with water more slowly compared to calcium, resulting in the formation of magnesium hydroxide and hydrogen gas.
Explore these reactions further to understand the dynamics and products involved when metals are introduced to water.
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