### Iodine Production ReactionIodine is made by the following reaction:\[ 2 \text{NaIO}_3(aq) + 5 \text{NaHSO}_3(aq) \rightarrow 3 \text{NaHSO}_4(aq) + 2 \text{Na}_2\text{SO}_4(aq) + \text{H}_2\text{O}(\ell) + \text{I}_2(aq) \]a. **Name the two reactants.** - **NaIO\(_3\)**: [Input Field] - **NaHSO\(_3\)**: [Input Field]b. **If you wish to prepare 2.11 kg of I\(_2\), what masses of NaIO\(_3\) and NaHSO\(_3\) are required?** - **Mass =** [Input Field] **g NaIO\(_3\)** - **Mass =** [Input Field] **g NaHSO\(_3\)**c. **What is the theoretical yield of I\(_2\) if you mixed 12.0 g of NaIO\(_3\) with 195 mL of 0.853 M NaHSO\(_3\)?** - **[Input Field] g I\(_2\)**### Explanation of the Problem#### Part a: Identifying ReactantsIn the reaction, the reactants are Sodium Iodate (NaIO\(_3\)) and Sodium Bisulfite (NaHSO\(_3\)). You need to provide their names in the input fields.#### Part b: Mass Calculations for Desired Product YieldTo calculate the masses needed to produce 2.11 kg of Iodine (I\(_2\)), you must use stoichiometry based on the balanced chemical equation. This involves converting the mass of I\(_2\) to moles, then using the mole ratio to find the required moles of each reactant, and converting these amounts back to grams.#### Part c: Theoretical Yield CalculationFor this section, you mix a given mass of NaIO\(_3\) with a solution of NaHSO\(_3\) to determine the theoretical yield of I\(_2\). You need to:1. Convert

Iodine is made by the following reaction 2 NaIO3(aq) + 5 NaHSO3(aq) → 3 NaHSO4 (aq) + 2 Na2SO4 (aq) + +H2O(l)+Iz(aq) a. Name the two reactants. NaIO3: NaHSO3: b. If you wish to prepare 2.11 kg of I2, what masses of NaIO3 and NaHSO3 are required? Mass= g NaIO 3 g NaHSO3 c. What is the theoretical yield of I2 if you mixed 12.0 g of NaIO3 with 195 mL of 0.853 M NaHSO3? Mass=

Iodine is made by the following reaction 2 NaIO3(aq) + 5 NaHSO3(aq) → 3 NaHSO4 (aq) + 2 Na2SO4 (aq) + +H2O(l)+Iz(aq) a. Name the two reactants. NaIO3: NaHSO3: b. If you wish to prepare 2.11 kg of I2, what masses of NaIO3 and NaHSO3 are required? Mass= g NaIO 3 g NaHSO3 c. What is the theoretical yield of I2 if you mixed 12.0 g of NaIO3 with 195 mL of 0.853 M NaHSO3? Mass=

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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Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

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### Iodine Production Reaction

Iodine is made by the following reaction:
\[ 2 \text{NaIO}_3(aq) + 5 \text{NaHSO}_3(aq) \rightarrow 3 \text{NaHSO}_4(aq) + 2 \text{Na}_2\text{SO}_4(aq) + \text{H}_2\text{O}(\ell) + \text{I}_2(aq) \]

a. **Name the two reactants.**
- **NaIO\(_3\)**: [Input Field]
- **NaHSO\(_3\)**: [Input Field]

b. **If you wish to prepare 2.11 kg of I\(_2\), what masses of NaIO\(_3\) and NaHSO\(_3\) are required?**
- **Mass =** [Input Field] **g NaIO\(_3\)**
- **Mass =** [Input Field] **g NaHSO\(_3\)**

c. **What is the theoretical yield of I\(_2\) if you mixed 12.0 g of NaIO\(_3\) with 195 mL of 0.853 M NaHSO\(_3\)?**
- **[Input Field] g I\(_2\)**

### Explanation of the Problem

#### Part a: Identifying Reactants
In the reaction, the reactants are Sodium Iodate (NaIO\(_3\)) and Sodium Bisulfite (NaHSO\(_3\)). You need to provide their names in the input fields.

#### Part b: Mass Calculations for Desired Product Yield
To calculate the masses needed to produce 2.11 kg of Iodine (I\(_2\)), you must use stoichiometry based on the balanced chemical equation. This involves converting the mass of I\(_2\) to moles, then using the mole ratio to find the required moles of each reactant, and converting these amounts back to grams.

#### Part c: Theoretical Yield Calculation
For this section, you mix a given mass of NaIO\(_3\) with a solution of NaHSO\(_3\) to determine the theoretical yield of I\(_2\). You need to:
1. Convert

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