How much solid product is expected when 12.06 g of FeS reacts with excess acid according to the following reaction? FeS(s) + 2 HCI(aq) → FeCl2(s) + H2S(g)
How much solid product is expected when 12.06 g of FeS reacts with excess acid according to the following reaction? FeS(s) + 2 HCI(aq) → FeCl2(s) + H2S(g)
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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![**Determining the Amount of Solid Product from a Reaction**
**Problem Statement:**
Calculate the amount of solid product expected when 12.06 g of FeS reacts with excess acid according to the following chemical reaction:
\[ \text{FeS(s)} + 2 \text{HCl(aq)} \rightarrow \text{FeCl}_2\text{(s)} + \text{H}_2\text{S(g)} \]
**Details:**
- **Given:** 12.06 grams of FeS.
- **Reaction:** Iron(II) sulfide (FeS) reacts with hydrochloric acid (HCl) to form iron(II) chloride (FeCl₂) and hydrogen sulfide gas (H₂S).
**Calculation Box:**
[Calculation Box Placeholders]
This problem involves stoichiometric calculations to determine the mass of FeCl₂ formed from a given mass of FeS when the reaction goes to completion with excess HCl provided.
The approach to solve this problem involves the following steps:
1. Calculate the molar mass of FeS.
2. Convert grams of FeS to moles using its molar mass.
3. Use the stoichiometric coefficients from the balanced equation to relate moles of FeS to moles of FeCl₂.
4. Calculate the mass of FeCl₂ produced using its molar mass.
To aid in calculation, you would also need the molar masses of the compounds involved:
- Molar mass of FeS.
- Molar mass of FeCl₂.
**Note:** Insert the calculated values and formulae appropriately in the calculation box.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19b0aed3-745e-4879-8577-ea35399669d0%2F6f100e93-b139-4358-9546-46108707b4c1%2F2jrn8ba_processed.png&w=3840&q=75)
Transcribed Image Text:**Determining the Amount of Solid Product from a Reaction**
**Problem Statement:**
Calculate the amount of solid product expected when 12.06 g of FeS reacts with excess acid according to the following chemical reaction:
\[ \text{FeS(s)} + 2 \text{HCl(aq)} \rightarrow \text{FeCl}_2\text{(s)} + \text{H}_2\text{S(g)} \]
**Details:**
- **Given:** 12.06 grams of FeS.
- **Reaction:** Iron(II) sulfide (FeS) reacts with hydrochloric acid (HCl) to form iron(II) chloride (FeCl₂) and hydrogen sulfide gas (H₂S).
**Calculation Box:**
[Calculation Box Placeholders]
This problem involves stoichiometric calculations to determine the mass of FeCl₂ formed from a given mass of FeS when the reaction goes to completion with excess HCl provided.
The approach to solve this problem involves the following steps:
1. Calculate the molar mass of FeS.
2. Convert grams of FeS to moles using its molar mass.
3. Use the stoichiometric coefficients from the balanced equation to relate moles of FeS to moles of FeCl₂.
4. Calculate the mass of FeCl₂ produced using its molar mass.
To aid in calculation, you would also need the molar masses of the compounds involved:
- Molar mass of FeS.
- Molar mass of FeCl₂.
**Note:** Insert the calculated values and formulae appropriately in the calculation box.
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