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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Transcribed Image Text:**Transcription for Educational Website**
1) Why is hydrochloric acid not used directly in a reaction with copper metal to produce CuCl₂?
2) What is the maximum amount of CuCl which can be produced by the procedure in this experiment if one starts with 1 g of copper metal?
3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced.
![### Chemical Reaction Equations
#### Equation 1
\[ \text{Cu}_{(s)} + 4 \text{H}^+_{(aq)} + 2 \text{NO}_3^-_{(aq)} \rightarrow \text{Cu}^{2+}_{(aq)} + 2 \text{NO}_2_{(g)} + 2 \text{H}_2\text{O} \]
#### Equation 2
\[ 2 \text{H}^+_{(aq)} + \text{CO}_3^{2-}_{(aq)} \rightarrow \text{H}_2\text{CO}_3_{(aq)} \rightarrow \text{CO}_2_{(g)} + \text{H}_2\text{O} \]
#### Equation 3
\[ \text{Cu}^{2+}_{(aq)} + \text{CO}_3^{2-}_{(aq)} \rightarrow \text{CuCO}_3(s) \]
#### Equation 4
\[ \text{CuCO}_3(s) + 2 \text{H}^+_{(aq)} + 4 \text{Cl}^-_{(aq)} \rightarrow \text{CuCl}_4^{2-}_{(aq)} + \text{CO}_2_{(g)} + \text{H}_2\text{O} \]
#### Equation 5
\[ \text{CuCl}_4^{2-}_{(aq)} + 4 \text{Cl}^-_{(aq)} \rightarrow 2 \text{CuCl}_3^-_{(aq)} \]
#### Equation 6
\[ \text{CuCl}_4^{2-}_{(aq)} \rightarrow \text{CuCl}_{(s)} + 3 \text{Cl}^-_{(aq)} \]
### Explanation
These equations represent a series of chemical reactions involving copper (Cu) compounds and various ions in aqueous solutions. The reactions illustrate typical transformations involving oxidation-reduction, precipitation, and complex ion formation. The processes include gaseous byproducts such as \(\text{NO}_2\) and \(\text{CO}_2\), and the use of acids to drive the reactions forward.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07988e83-a3e9-4d52-ab01-33c4f0c30b8b%2F4f75fcb6-0c23-4dac-8b88-80cfc70ef07f%2Fh9cl0fg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Equations
#### Equation 1
\[ \text{Cu}_{(s)} + 4 \text{H}^+_{(aq)} + 2 \text{NO}_3^-_{(aq)} \rightarrow \text{Cu}^{2+}_{(aq)} + 2 \text{NO}_2_{(g)} + 2 \text{H}_2\text{O} \]
#### Equation 2
\[ 2 \text{H}^+_{(aq)} + \text{CO}_3^{2-}_{(aq)} \rightarrow \text{H}_2\text{CO}_3_{(aq)} \rightarrow \text{CO}_2_{(g)} + \text{H}_2\text{O} \]
#### Equation 3
\[ \text{Cu}^{2+}_{(aq)} + \text{CO}_3^{2-}_{(aq)} \rightarrow \text{CuCO}_3(s) \]
#### Equation 4
\[ \text{CuCO}_3(s) + 2 \text{H}^+_{(aq)} + 4 \text{Cl}^-_{(aq)} \rightarrow \text{CuCl}_4^{2-}_{(aq)} + \text{CO}_2_{(g)} + \text{H}_2\text{O} \]
#### Equation 5
\[ \text{CuCl}_4^{2-}_{(aq)} + 4 \text{Cl}^-_{(aq)} \rightarrow 2 \text{CuCl}_3^-_{(aq)} \]
#### Equation 6
\[ \text{CuCl}_4^{2-}_{(aq)} \rightarrow \text{CuCl}_{(s)} + 3 \text{Cl}^-_{(aq)} \]
### Explanation
These equations represent a series of chemical reactions involving copper (Cu) compounds and various ions in aqueous solutions. The reactions illustrate typical transformations involving oxidation-reduction, precipitation, and complex ion formation. The processes include gaseous byproducts such as \(\text{NO}_2\) and \(\text{CO}_2\), and the use of acids to drive the reactions forward.
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