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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how do you find the oxidizing agent and reducing agent for the following chemical equations?
![Here are the chemical reactions depicted in the image:
1. **Reaction of Potassium Dichromate with Sodium Nitrite:**
\[
K_2Cr_2O_7 + NaNO_2 \xrightarrow{H_2SO_4} Cr^{3+} + NO
\]
In this reaction, potassium dichromate (\(K_2Cr_2O_7\)) reacts with sodium nitrite (\(NaNO_2\)) in the presence of sulfuric acid (\(H_2SO_4\)), resulting in chromium ions (\(Cr^{3+}\)) and nitric oxide (\(NO\)).
2. **Reaction of Potassium Dichromate with Iron(II) Sulfate:**
\[
K_2Cr_2O_7 + FeSO_4 \xrightarrow{H_2SO_4} Cr^{3+} + Fe^{3+}
\]
This reaction shows potassium dichromate (\(K_2Cr_2O_7\)) reacting with iron(II) sulfate (\(FeSO_4\)) in the presence of sulfuric acid (\(H_2SO_4\)), yielding chromium ions (\(Cr^{3+}\)) and iron(III) ions (\(Fe^{3+}\)).
3. **Reaction of Potassium Iodide with Nitric Acid:**
\[
KI + HNO_3 \rightarrow I_2
\]
Here, potassium iodide (\(KI\)) reacts with nitric acid (\(HNO_3\)), producing iodine (\(I_2\)).
These reactions illustrate redox processes where oxidizing agents such as potassium dichromate are used to oxidize other compounds, leading to the formation of different ionic species.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F173cfd6c-bb08-42c3-aae4-d18dc2eee3ee%2Ffa0bfaa4-716c-437b-9801-8852b41c2887%2Fpiupgji_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Here are the chemical reactions depicted in the image:
1. **Reaction of Potassium Dichromate with Sodium Nitrite:**
\[
K_2Cr_2O_7 + NaNO_2 \xrightarrow{H_2SO_4} Cr^{3+} + NO
\]
In this reaction, potassium dichromate (\(K_2Cr_2O_7\)) reacts with sodium nitrite (\(NaNO_2\)) in the presence of sulfuric acid (\(H_2SO_4\)), resulting in chromium ions (\(Cr^{3+}\)) and nitric oxide (\(NO\)).
2. **Reaction of Potassium Dichromate with Iron(II) Sulfate:**
\[
K_2Cr_2O_7 + FeSO_4 \xrightarrow{H_2SO_4} Cr^{3+} + Fe^{3+}
\]
This reaction shows potassium dichromate (\(K_2Cr_2O_7\)) reacting with iron(II) sulfate (\(FeSO_4\)) in the presence of sulfuric acid (\(H_2SO_4\)), yielding chromium ions (\(Cr^{3+}\)) and iron(III) ions (\(Fe^{3+}\)).
3. **Reaction of Potassium Iodide with Nitric Acid:**
\[
KI + HNO_3 \rightarrow I_2
\]
Here, potassium iodide (\(KI\)) reacts with nitric acid (\(HNO_3\)), producing iodine (\(I_2\)).
These reactions illustrate redox processes where oxidizing agents such as potassium dichromate are used to oxidize other compounds, leading to the formation of different ionic species.
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