**Ch 7 Homework****Problem-Solving Strategies: Understanding Equilibrium**For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase:\[ \text{NH}_3(g) + \text{H}_2\text{O}(l) \rightleftharpoons \text{NH}_4^+ (aq) + \text{OH}^- (aq) \]**Instructions:** Drag the appropriate stresses to their respective bins.**Options:**- Removing $\text{NH}_4^+$ (aq)- Removing $\text{OH}^-$ (aq)- Adding $\text{OH}^-$ (aq)- Adding $\text{NH}_3(g)$- Adding $\text{NH}_4^+$ (aq)**Bins:**- Shift in the direction of the reactants- Shift in the direction of the products**Buttons:**- Reset- Help**Action:** [Submit Button] **Problem-Solving Strategies: Understanding Equilibrium**### Part A - Identify the StressConsider the equilibrium reaction:\[ \text{CO}(g) + \text{H}_2\text{O}(g) \leftrightarrow \text{CO}_2(g) + \text{H}_2(g) \]Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response.**Instructions:** Drag the appropriate labels to their respective targets.**Options:**- **Increase reactant**: Reverse reaction rate temporarily increases.- **Decrease reactant**: Forward reaction rate temporarily increases.- **Increase product**: Forward reaction rate temporarily decreases.- **Decrease product**: Reverse reaction rate temporarily decreases.**Diagram Explanation:**The diagram is divided into three columns:1. **Change** - This column lists possible changes to the system: - Add CO(g) - Remove H₂O(g) - Add CO₂(g) - Remove H₂(g)2. **System stress** - This column has placeholders for "Group 1."3. **Equilibrium shift** - This column has placeholders for "Group 2."**Controls:**- **Reset**: Start over with the options and selections.- **Help**: Access hints or additional information.Finally, there is a "Submit" button to confirm your selections.

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em-Solving Strategies: Understanding Equilibrium For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g) + H₂O(1) NH₂ (aq) + OH-(aq) Drag the appropriate stresses to their respective bins. ► View Available Hint(s) Removing NH₂ (aq) Removing OH (aq) Shift in the direction of the reactants Adding OH (aq) Adding NH3(g) Adding NH₂ (aq) Shift in the direction of the products Reset Help

em-Solving Strategies: Understanding Equilibrium For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g) + H₂O(1) NH₂ (aq) + OH-(aq) Drag the appropriate stresses to their respective bins. ► View Available Hint(s) Removing NH₂ (aq) Removing OH (aq) Shift in the direction of the reactants Adding OH (aq) Adding NH3(g) Adding NH₂ (aq) Shift in the direction of the products Reset Help

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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For the following systems at equilibrium A: 2NOCI(g) B: H2(g) +I2(g) = 2NO(g)+Cl2 (g) = 2HI(g) classify these changes by their effect. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help System A Increase container size System A Decrease container size System B Increase container size System B Decrease container size Leftward shift No shift Rightward shift
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A аpp.101еdu.co Update Question 7 of 11 Submit The reaction 2C0(g) + MoO2(s) = CO2(g) +Mo(s) is reaching equilibrium. How would increase the volume of the container affects the reaction? A) The equilibrium of this reaction wilImove forward (to the right). B) The equilibrium of this reaction will move backward (to the left). C) The equilibrium of this reaction will not change. D) The equilibrium of this reaction can not be decided. 11165 A W Air F10 F11 F12 F8 F9 8 { P. + I|
CHEMWORK For the following endothermic reaction system at equilibrium: 2S03(g) 2 2SO,(g)+ O2(g) Choose the changes that will increase the value of K. (Select all that apply.) Remove SO3(g) (constant T) O Add SO,(g) (constant T) Increase the temperature Decrease the temperature ODecrease the volume (constant T) ot Add a catalyst (constant T) U Add Ne(g) (constant T) ot An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer. ot ot Submit Show Hints pt pt Submit Answer Try Another Version 7 item attempts remaining pt
MISSED THIS? Read Section Predict the effect (shift right, shift left, or no effect) of decreasing the reaction temperature. 16.9 (Pages 711-718); Watch KCV 16.9. The following reaction is endothermic. C (s) + CO2 (g) = 2 CO (g) O no effect O shifts right O shifts left Submit Request Answer Part D How does the value of the equilibrium constant from the previous part depend on temperature? O K does not change O K increases O K decreases
Initial (M) Change (M) Equilibrium (M) -2.0 Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H2, 8.0 M N₂, and 4.0 M NH3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 0 2.0 5.0 N₂(g) + 3 H₂(g) = 2 NH3(g) -5.0 N₂(g) Ssivestit 8.0 1 6.0 + 4.0 -6.0 3 H₂(g) ઇસ્કો અને કોની -4.0 10 10.0 2 NH3(g) RESET 11.0
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6.B Consider the chemical equation A(aq) + 3B(aq) 5 2C(aq) with an equilibrium constant equal to 4.00 at a certain temperature. Each chemical is initially present at a concentration of 0.25 molar. (a) Set up a simple* expression for the equilibrium constant. (*freshman level) (b) Determine whether the forward or reverse reaction is occurring. (c) Set up an 1CE table to begin a calculation of the equilibrium composition. (d) Without a better calculator or resources on the internet, you cannot solve for the equilibrium composition. Which value for "x" works: 0.0261, 0.0315, or - 0.0129. If they all fail, then one of us did something wrong.
mal resources @ 2 Predict the equilibrium concentration of O₂ in the reaction described below by constructing an equilibrium expression for Qc, constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. N₂(g) + O₂(g) = 2 NO(g) [0] [0.050] NEXT > In a 1.0 L container at high temperature, 0.20 mol N₂ and 0.15 mol O₂ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. 0.030 # 3 [1.0] [0.20]² 9.0 x 10-4 1 $ 4 Qc = [0]² [0.15]² 1.1 x 10² 25 2 % Question 4 of 7 [1.0]² ... [0.40]² ^ 6 3 [0.20] [0.30]² & 7 = * [0.15] [0.050]² 8 4 ( 9 [0.40] 0 ) RESET [0.30] 33 +
AutoSave CHEM 212 Final Exam_Fall 2020 Word Search 困 ff steve M SM File Home Insert Draw Design Layout References Mailings Review View Help E Share O Comments 3a) Calculate AGon for this reaction: CH3OH (g) → CO (g) + 2 H2 (g) The equilibrium partial pressures for each component are: CH;OH = 0.620 atm, CO = 0.105 atm, H2 = 0.125 atm b) Is the reaction spontaneous? Briefly explain. 3c) Cells use the hydrolysis of adenosine triphosphate (ATP) as a source of energy. The conversion of ATP to ADP has a standard free energy change of -30.5 kJ/mol. If all the free energy from the metabolism of glucose goes to the conversion of ADP to ATP, how many mole of ATP can be produced for each mole of glucose? Page 3 of 6 492 words D Focus 80%