Anyone check （step by step）if my chem balance is written correctly？ The image contains handwritten chemical equations relating to the reaction of arsenic in acid:1. **Equation (Unbalanced)**: \[ \text{As(s)} + \text{ClO}_3^-(aq) \rightarrow \text{H}_3\text{AsO}_3(aq) + \text{HClO}_2(aq) \] This equation represents the reaction between solid arsenic (As) and chlorate ions (\( \text{ClO}_3^- \)) in aqueous solution, producing arsenous acid (\( \text{H}_3\text{AsO}_3 \)) and chlorous acid (\( \text{HClO}_2 \)).2. **Balanced Equation**: \[ \text{As} + \text{ClO}_3^- + 4\text{H}^+ \rightarrow \text{As} + 3\text{ClO} + \text{H}_4\text{O}_3 \] A balanced version of the reaction includes hydrogen ions (\( \text{H}^+ \)) indicating the acidic conditions. This balance reflects the stoichiometry necessary for conservation of mass and charge.There is an indication that this second equation is marked as balanced, suggesting the intention to show the correct stoichiometric coefficients required for a balanced chemical equation under acidic conditions.No graphs or diagrams are present in the image; only textual chemical equations.

Answered: in acid) balanced ÅStcloz+4H> As…

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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Anyone check （step by step）if my chem balance is written correctly？

The image contains handwritten chemical equations relating to the reaction of arsenic in acid:

1. **Equation (Unbalanced)**:
\[
\text{As(s)} + \text{ClO}_3^-(aq) \rightarrow \text{H}_3\text{AsO}_3(aq) + \text{HClO}_2(aq)
\]
This equation represents the reaction between solid arsenic (As) and chlorate ions (\( \text{ClO}_3^- \)) in aqueous solution, producing arsenous acid (\( \text{H}_3\text{AsO}_3 \)) and chlorous acid (\( \text{HClO}_2 \)).

2. **Balanced Equation**:
\[
\text{As} + \text{ClO}_3^- + 4\text{H}^+ \rightarrow \text{As} + 3\text{ClO} + \text{H}_4\text{O}_3
\]
A balanced version of the reaction includes hydrogen ions (\( \text{H}^+ \)) indicating the acidic conditions. This balance reflects the stoichiometry necessary for conservation of mass and charge.

There is an indication that this second equation is marked as balanced, suggesting the intention to show the correct stoichiometric coefficients required for a balanced chemical equation under acidic conditions.

No graphs or diagrams are present in the image; only textual chemical equations.

Expert Solution

Step 1

In the given redox reaction, the oxidation state of As increases from 0 in As to +3 in H₃AsO₃. Increase in oxidation number signifies oxidation. Hence, As is being oxidized. On the other hand, the oxidation state of Cl decreases from +5 in ClO₃^- to +1 in HClO. Decrease in oxidation number is called as reduction. Hence, chlorine is being reduced in the redox reaction. The balancing of a redox reaction in acidic medium by ion-electron method involves following steps:

The reaction is split into oxidation-half reaction and reduction-half reaction.
The atoms of each half reaction are balanced (excluding O and H).
Hydrogen and oxygen atoms are balanced after balancing the other atoms. In acidic or neutral medium, water molecule is added on the side deficient in oxygen and hydrogen ion is added to the side deficient in hydrogen.
Electrons are added on the side deficient in electrons.
The number of electrons is equalized in both the reactions by multiplying a suitable number.
The two balanced half reactions are added and the common terms are cancelled on the opposite sides.

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