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3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced..

3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced..

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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**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.
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.
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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