**Chemistry Problem: Calculating Moles of Silver Produced**Solid silver can be produced by reacting silver (I) nitrate with copper according to the reaction below. How many moles of silver can be produced if 0.111 moles of Cu was placed in silver (I) nitrate solution? (Assume the AgNO₃ is in excess.)**Chemical Reaction:**\[ \text{Cu(s)} + 2 \text{AgNO}_3\text{(aq)} \rightarrow \text{Cu(NO}_3\text{)}_2\text{(aq)} + 2 \text{Ag(s)} \]**Your Answer:**| | ||------------------|-----------|| **Answer** | **units** |**Explanation:**This problem requires the application of stoichiometry to determine the amount of silver produced. In the given reaction, one mole of copper (Cu) reacts with two moles of silver nitrate (AgNO₃) to produce two moles of silver (Ag). The presence of excess silver nitrate ensures that all of the copper will be used in the reaction. Therefore, the moles of silver produced will be double the moles of copper used.- **Given:** 0.111 moles of copper (Cu)- **Find:** Moles of silver (Ag)Since the reaction shows that 1 mole of Cu produces 2 moles of Ag, you can calculate the moles of Ag by multiplying the moles of Cu by 2.

Given chemical reaction : Cu + AgNO3 ---> Cu(NO3)2 + Ag Moles of Cu = 0.111

Answered: was placed in silver (I) nitrate…

was placed in silver (I) nitrate solution (Assume the AGNO3 is in excess)? Cu(s) + 2 AGNO3(aq)→ Cu(NO3)2(aq) + 2 Ag(s) Your Answer: Answer units

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

**Chemistry Problem: Calculating Moles of Silver Produced**

Solid silver can be produced by reacting silver (I) nitrate with copper according to the reaction below. How many moles of silver can be produced if 0.111 moles of Cu was placed in silver (I) nitrate solution? (Assume the AgNO₃ is in excess.)

**Chemical Reaction:**

\[ \text{Cu(s)} + 2 \text{AgNO}_3\text{(aq)} \rightarrow \text{Cu(NO}_3\text{)}_2\text{(aq)} + 2 \text{Ag(s)} \]

**Your Answer:**

| | |
|------------------|-----------|
| **Answer** | **units** |

**Explanation:**

This problem requires the application of stoichiometry to determine the amount of silver produced. In the given reaction, one mole of copper (Cu) reacts with two moles of silver nitrate (AgNO₃) to produce two moles of silver (Ag). The presence of excess silver nitrate ensures that all of the copper will be used in the reaction. Therefore, the moles of silver produced will be double the moles of copper used.

- **Given:** 0.111 moles of copper (Cu)
- **Find:** Moles of silver (Ag)

Since the reaction shows that 1 mole of Cu produces 2 moles of Ag, you can calculate the moles of Ag by multiplying the moles of Cu by 2.

Expert Solution

Step 1

Given chemical reaction :

Cu + AgNO₃ ---> Cu(NO₃)₂ + Ag

Moles of Cu = 0.111

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