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=

Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter4: Chemical Reactions
Section: Chapter Questions
Problem 4.100P
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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
Transcribed Image Text:### 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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