nical Equilibrium: Data Sheet Fill in the following table: Substance Equilibrium shifted towards Equilibrium shifted towards Test added Color Trial 2 Color Trial 1 tube Temperature change Reference Reference color: Reference lo drops waley 1 8 drops Fe CNO3) Dark Red Dak Red. Foruword ReacHon Forcward Reocthion Forword 8 drops KSCN Donk Red Dank Red Forword Reaction 3 Reaction Backword Light Oronge Orange Backward clirecion 8 drops Light 4. direction HCI lo drops Light Oronge Forward Reachon Fonvord Reachion Light o 1onge H0+ Heat Fonward lo drops Ha0+ Cad Doik Red Dork Oionge Forward Red 6 Reaction Reachon Questions: 1. Show calculations for making the 0.01 M solutions of Fe(NO3)3 and KSCN. M,VI= M2VZ M.VI M2 V2 1.0XV, 3 0-0lx SO = O.5 ML : 0-5 mL Fe(NOs)s KSCIN 2. Based on test tubes 5 and 6, is the forward reaction of the equilibrium exothermic or endothermic? Hint: add heat to the reaction below as a product and reactant and see which make sense with your results. Fe* (aq) + SCN (aq) FESCN²* (aq)
nical Equilibrium: Data Sheet Fill in the following table: Substance Equilibrium shifted towards Equilibrium shifted towards Test added Color Trial 2 Color Trial 1 tube Temperature change Reference Reference color: Reference lo drops waley 1 8 drops Fe CNO3) Dark Red Dak Red. Foruword ReacHon Forcward Reocthion Forword 8 drops KSCN Donk Red Dank Red Forword Reaction 3 Reaction Backword Light Oronge Orange Backward clirecion 8 drops Light 4. direction HCI lo drops Light Oronge Forward Reachon Fonvord Reachion Light o 1onge H0+ Heat Fonward lo drops Ha0+ Cad Doik Red Dork Oionge Forward Red 6 Reaction Reachon Questions: 1. Show calculations for making the 0.01 M solutions of Fe(NO3)3 and KSCN. M,VI= M2VZ M.VI M2 V2 1.0XV, 3 0-0lx SO = O.5 ML : 0-5 mL Fe(NOs)s KSCIN 2. Based on test tubes 5 and 6, is the forward reaction of the equilibrium exothermic or endothermic? Hint: add heat to the reaction below as a product and reactant and see which make sense with your results. Fe* (aq) + SCN (aq) FESCN²* (aq)
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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I need help in doing homework
Can someone please check my work.
![**Chemical Equilibrium: Data Sheet**
**Experiment Table:**
| Test Tube | Substance Added /Temperature Change | Color Trial 1 | Color Trial 2 | Equilibrium Shifted Towards | Equilibrium Shifted Towards |
|-----------|------------------------------------|-----------------|---------------|-----------------------------|-----------------------------|
| 1 | 10 drops water | Reference color | | Reference | Reference |
| 2 | 8 drops Fe(NO₃)₃ | Dark Red | Dark Red | Forward Reaction | Forward Reaction |
| 3 | 8 drops KSCN | Dark Red | Dark Red | Forward Reaction | Forward Reaction |
| 4 | 8 drops HCl | Light Orange | Light Orange | Backward Reaction | Backward Reaction |
| 5 | 10 drops H₂O + Heat | Light Orange | Light Orange | Forward Reaction | Forward Reaction |
| 6 | 10 drops H₂O + Cold | Dark Red | Dark Orange | Forward Reaction | Forward Reaction |
**Questions:**
1. **Show Calculations for Making the 0.01 M Solutions of Fe(NO₃)₃ and KSCN:**
- **Fe(NO₃)₃ Calculation:**
\[
M_1V_1 = M_2V_2
\]
\[
1.0 \times V_1 = 0.01 \times 50
\]
\[
V_1 = 0.5 \, \text{mL} \, \, \text{Fe(NO₃)₃}
\]
- **KSCN Calculation:**
\[
M_1V_1 = M_2V_2
\]
\[
1.0 \times V_1 = 0.01 \times 50
\]
\[
V_1 = 0.5 \, \text{mL} \, \, \text{KSCN}
\]
2. **Based on Test Tubes 5 and 6, is the Forward Reaction of the Equilibrium Exothermic or Endothermic?**
**Hint](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F81ac168b-024d-494f-99de-3f3384ea3f4e%2F39071088-8646-411a-92f6-d71a92db5084%2F8wtaral_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium: Data Sheet**
**Experiment Table:**
| Test Tube | Substance Added /Temperature Change | Color Trial 1 | Color Trial 2 | Equilibrium Shifted Towards | Equilibrium Shifted Towards |
|-----------|------------------------------------|-----------------|---------------|-----------------------------|-----------------------------|
| 1 | 10 drops water | Reference color | | Reference | Reference |
| 2 | 8 drops Fe(NO₃)₃ | Dark Red | Dark Red | Forward Reaction | Forward Reaction |
| 3 | 8 drops KSCN | Dark Red | Dark Red | Forward Reaction | Forward Reaction |
| 4 | 8 drops HCl | Light Orange | Light Orange | Backward Reaction | Backward Reaction |
| 5 | 10 drops H₂O + Heat | Light Orange | Light Orange | Forward Reaction | Forward Reaction |
| 6 | 10 drops H₂O + Cold | Dark Red | Dark Orange | Forward Reaction | Forward Reaction |
**Questions:**
1. **Show Calculations for Making the 0.01 M Solutions of Fe(NO₃)₃ and KSCN:**
- **Fe(NO₃)₃ Calculation:**
\[
M_1V_1 = M_2V_2
\]
\[
1.0 \times V_1 = 0.01 \times 50
\]
\[
V_1 = 0.5 \, \text{mL} \, \, \text{Fe(NO₃)₃}
\]
- **KSCN Calculation:**
\[
M_1V_1 = M_2V_2
\]
\[
1.0 \times V_1 = 0.01 \times 50
\]
\[
V_1 = 0.5 \, \text{mL} \, \, \text{KSCN}
\]
2. **Based on Test Tubes 5 and 6, is the Forward Reaction of the Equilibrium Exothermic or Endothermic?**
**Hint

Transcribed Image Text:**Chemical Equilibrium**
**Objective**
To observe and explain equilibrium shifts based on Le Chatelier’s Principle.
**Introduction**
In any chemical reaction, reactants are converted to products. In some cases, some of the products are converted back to reactants. Such reactions are called reversible reactions where reactants are converted to products (forward reaction) and products are converted back to reactants (reverse reaction). When the rate of the forward reaction becomes equal to the rate of the reverse reaction, we say that the reaction is at equilibrium. At this point, there is no change in the concentration of the reactants and the products.
We can disturb a reaction at equilibrium by changing the concentration, pressure/volume or temperature. Le Chatelier’s Principle states that a reaction (system) at equilibrium will stay at equilibrium until acted upon by some outside force that changes the equilibrium conditions—for example, by adding a greater concentration of one of the products or reactants. The system will then adjust to return to equilibrium by counteracting the change that has just been made.
Some examples of stresses and how the equilibrium system responds to counteract those stresses are as follows:
**Change in Concentration**
- If we add a reactant, the equilibrium will shift towards the products. This is because a portion of the added reactant will be used up to form more products, until the equilibrium is re-established.
- If we remove a reactant, then to compensate for the loss of the reactants, the product will decompose to form reactants and therefore the equilibrium will shift towards the reactants.
- If we add a product, then the equilibrium will shift to the reactants in order to consume the excess product.
- If we remove a product, then to compensate for the loss of the products, more product will be formed from the reactants and the equilibrium will also shift towards the products.
**Changes in Temperature**
- An endothermic process will be favored (shifting towards the formation of products) by an increase in temperature. The reaction shifts in the direction that absorbs heat to counteract the increase in temperature.
- An exothermic process will be favored (shifting towards the formation of products) by a decrease in temperature. The reaction shifts in the direction that releases heat to counteract the decrease in temperature.
During this lab, you will investigate Le Chatelier’s Principle using iron(III)-thiocyanate equilibrium. You will be combining Fe(NO₃)
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