Spring 2023 CHEM 120-Det of Eq Constants-Post Lab Q-M-Th Final v2

Write the basic equilibrium equation for (CH3)2NH. Be sure to include the proper phases for all species within the reaction. 1 U + 4 2 0₂ Reset ( H₂O 3 ) 4 5 → (CH3)2NH OH- 5 6 6 (s) 2+ 7 N H3O+ 3+ 4+ 8 9 0 ☐o (1) • H₂O 9 (g)) (aq) H Delete

this is an ungraded question please help me.

Table 1: Absorbance data recorded for five 0.200 M Fe(NO:)3 solutions at 20.0 °C Beaker 0.0020 M [FESCN2+] (M) Abs. 0.00200 SCN (mL) Fe(NO3)3 (mL) 5.0 0.00 0.00 M -0.001 2 5.0 2.00 8.0 x 10-5 M 0.278 5.0 3.00 1.2 x 10-4 M 0.415 4 5.0 4.00 1.6 x 10-4 M 0.555 5.0 5.00 2.0 x 10-4 M 0.671 Part 1: y=3386x+0.0043 R^2=0.9991 Part II – Determining Concentration of an Unknown Table 2: Best-fit line and Absorbance data of unknown solution Best-fit line equation from Part I Absorbance reading of unknown 0.338 Part III – Determining the Equilibrium Constant Test tube 0.0020 M 0.00200 H20 (mL) Abs. Net Abs Fe(NO3)3 (mL) SCN-(mL) 1 3.00 0.00 7.00 0.000 2 3.00 2.00 5.00 0.119 0.119 3 3.00 3.00 4.00 0.212 0.212 4 3.00 4.00 3.00 0.265 0.265 5 3.00 5.00 2.00 0.335 0.335

3. Consider the equilibrium that you studied in this experiment: Fe (aq) + SCN (aq) FESCN²* (aq) Direction of shift (copy from previous Type of stress (ex: reactant Test Tube added, product removed, temp inc) Explain how the direction of shift relieves the applied stress. page) Forward Reaction Forword Reaction 3 Backword 4 Peaction Backword Reac Hon Fonword Reachion

the progress with time of a reaction system is depicted in the figure here. Red spheres represent the molar concentration of substance A, and blue spheres represent the molar concentration of substance B. What is the value of the equilibrium constant Kc

Kinetics and Equilibrium Calculating an equilibrium constant from a heterogeneous equilibrium... Try Again Try again... Bis 2/5 Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. Fluoride anion and hydronium cation react to form hydrofluoric acid and water, like this: F (aq)+H3O (aq)→HF (aq) + H2O(l) At a certain temperature, a chemist finds that a 9.9 L reaction vessel containing an aqueous solution of fluoride anion, hydronium cation, hydrofluoric acid, and water at equilibrium has the following composition: compound amount F 0.146 g H₂O 0.364 g HF 4.96 g 892. g H₂O Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K 8.4 x 10 C

The 2 images attached go together so with the image attached please write 1 paragraph 1 paragraph: analysis explained in one paragraph Please please please answer everything it's very important please answer fast Please write it in one paragraph please

please help, im not sure if my part 1 and 2 are right.

Provide clear explanation and show work. Clear writing or typed please

Activity 1: Complete Me! Direction: Complete the following table. Write your answer on a separate sheet of paper. Equilibrium Reaction Effect Keq expression Stress Equilibrium shift (encircle your answer) Forward applied (encircle your answer) Ha + Cla = | 2HCI Decreasing the pressure (increase, decrease, no change) in the number (HCIJ Keq - Backward No Shift of moles of HCl(g) (increase, decrease, no change) in the volume of Increasing Fe,O +4 Ha + heat 2 Forward Keq = the Backward 3Fe + 4H,O temperature No Shift water vapor collected of (increase, decrease, no change) the number of moles of NO 2NO + Oz 2NO + heat Forward Backward No Shift Addition (NO,P |NO]F|0,]| Keq = helium Forward H,CO» = CO2 + H,O Removal of (increase, decrease, no change) in the amount Keq - (H,CO, CO2 Backward No Shift of H,CO, (increase, decrease, no change) in amount of o, (increase, the volume of decrease, no change) in the Increasing the Forward Backward No Shift Keq= temperature the 4 NH3%g + 502 2 4NO+ 6…

Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 2 NEXT > A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) + H₂O(l) = HsO-(aq) + A-(aq)

Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 2 NEXT > A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) H₂O(1) = H,O*(aq) A (aq)

Direction: Complete the following table. Write your answer on a separate sheet of раper. Effect (encircle your shift (encircle answer) (increase, Equilibrium Reaction Keq expression Stress Equilibrium applied your answer) Forward H2 + Cl2 2 2HCI (HCI]? Keq- Decreasing the pressure decrease, no Backward change) in the number No Shift of moles of HCl(g) (increase, decrease, no temperature change) in the volume of water Increasing the Forward FesO4(s) +4 H2) + heat 2 3Fee) + 4H2Og) [H,0]* [H2J* Keq Backward No Shift vapor collected of (increase, decrease, no change) in the number of moles of NO 2NO + O2ia) | 2NO2) + heat (NO, Keq (NO]?(0;] Addition helium Forward Backward No Shift

Determine the Kb for cocaine (a base) by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT > The pH for 6.1 x 104 M solution of cocaine, a weak base, is 9.60. Let cocaine be represented by the generic base, B. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) B(aq) + H₂O(1) 0 6.1 × 10-4 9.60 -4.0 x 10-5 2.1 × 10-4 -2.1 × 10-4 5.7 × 10-4 3 =4 OH(aq) + BH*(aq) RESET -9.60 2.5 x 10-10 -2.5 x 10-10 4.0 × 10-5 -5.7 × 10-4 Stv A

Equilibrium and Reversible Reactions Part A. Name: PhET Equilibrium Inquiry Activity Learning Goals 1) Visualize a system at dynamic equilibrium state (DES) 2) Characterize the DES by finding the red: green ball ratio, Krg. 3) Design an investigation to test the effect of changing temperature, number of balls and activation energy barrier has on the Part 1: Play Instructions: 1) Open the PhET "Reversible Reactions" simulation. (https://phet.colorado.edu/en/simulation/legacy/reversible-reactions) 2) Play with the simulation. Click on EVERYTHING! 3) Answer the following questions: I 1) Put some number of balls (>50) in one of the wells. In a table, record the number of green and red balls in each well as a function of time. (Suggested time length: 5 minutes, suggested intervals: 15-20 seconds) Paste the table into this document. (Google spreadsheet will work well for this.) 2) Paste in a graph of your data. Describe the shape of the graph and what it means in terms of the red and green…

Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) + H₂O(l) = H3O+ (aq) + A-(aq)

Review the reversible reactions given, along with the associated equilibrium constant K at room temperature. In each case, determine whether the forward or reverse reaction is favored. AgCl → Ag* + Cl'Ksp=1.6 x 1010 Choose... - A + B + CK=4.9 x 103 Choose... CH3COOH + CH3C00" + H*Kg=1.8 x 10-5 Choose... Alš+ + 30H Ksp=3.7 x 1015 Choose... - Choose... Reverse Forward Al(OH)3

Determine the pH of a solution of HCIO2 by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 A 0.020 M aqueous solution of HCIO2 is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) -2x 1.2 x 10-² - 2x 0 0.020 + x 1 HCIO₂(aq) 0.020 0.020 - x + 2 H₂O(l) 1.2 x 10-² 0.020 + 2x 0.010 0.020 - 2x H3O+ (aq) +X 1.2 x 10-² + x -X + NEXT 1.2 x 10-² - x CIO₂ (aq) RESET +2x 1.2 x 10-² + 2x >

Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O2 at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. 2 H2O(g) 2 H2(g) + O2(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 10-3 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [×] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Ко = = 2.4 × 10-3 RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]2

10.0 20.0 30.0 40.0 50.0 Use the References to ac O A. 1.9x10-4 M/min OB. 1.6x10-3 M/min O C. 2.2x10-3 M/min O D. 3.4x10-3 M/min O E. 7.8x10-4 M/min es it For the reaction 2 SO3 →→→→2 SO₂ + O₂, calculate the average rate, A[SO3]/At, between 20.0 min and 40.0 min for the loss of SO3. Time (min) [SO3], M [SO₂], M [0₂], M 0.0 0.0 0.124 0.0 0.092 0.032 0.016 0.068 0.056 0.028 0.050 0.074 0.037 0.037 0.087 0.044 0.028 0.096 0.048 ded for this question

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Predict the direction in which the equilibrium will lie for the reactionH2SO3(aq) + HCO3– (aq)  <->  HSO3–(aq) + H2CO3(aq).Ka1(H2SO3) = 1 × 10–2; Ka1(H2CO3) = 4.2 × 10–7

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Consider the following reaction: CO(g) + 2H2 (g) = CH3OH(g) The reaction between CO and H2 is carried out at a specific temperature with initial concentrations of CO = 0.29 M and H2 = 0.50 M.At equilibrium, the concentration of CH, OH is 0.16 M. Part A Find the equilibrium constant at this temperature. Express your answer using two significant figures. Ke = Submit Request Answer Provide Feedback MacBook Air F10 吕口 F3 F6 D00 F4 F5 esc EL F2