CHM 101L M5 Equilibrium and LeChatlier Lab Report

Consider the following equilibrium: Blank 12+ (aq) + 4Cl-(aq) =[BLANK-212- (aq) + 6H₂O (1) Which direction does the reaction shift by increasing the chloride ion concentration? Blank 1 Add your answer

What is the equilibrium constant expression for the reaction? CH3COOH + C2H5OH <======> CH3COOC2H5  + H2O

A chemical engineer is studying the following reaction: H2(g)+I½(g) → 2 HI(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.31. The engineer charges ("fills") three reaction vessels with hydrogen and iodine, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel H, 3.32 atm f increase I decrease (no change) A 3.04 atm f increase I decrease (no change) HI 0.76 atm f increase O I decrease (no change) H, 3.29 atm f increase I decrease (no change) В 3.01 atm f increase I decrease (no change) HI 0.81 atm f increase O 1 decrease O (no change)

(NH4)2CO3(s) 22 NH3(g) + CO2(g) + H2O(g) [(NH4)½CO3] [NH3] [CO2] [H2O] [H2O] [(NH4)2CO3] K. = [NH3] [CO2] Build the equilibrium constant expression for the reaction shown. Step 1. Drag the reactants and products to the numerator or denominator as appropriate. Click a species to remove it from the expression. Step 2. Drag the coefficients to the appropriate species. Click a coefficient to remove it from the expression. Recheck Next (5 of 8) 1?nd attemnt

Lactase is an enzyme that breaks down the sugar lactose which is commonly found in dairy products. Some people develop lactose intolerance as they grow older and the amount of lactase enzyme in their gut diminishes. Since the enzyme is commonly found in the gut of humans it can withstand a pH that is very acidic, ranging from a pH of 2-7. A student decided to do an experiment to determine how the pH of a solution affects lactase enzyme activity. Lactase works by breaking lactose into its two component sugars of glucose and galactose.   To conduct the experiment the student prepared a solution of lactose and placed it into 5 different test tubes. A pH buffer solution was then added to each test tube with a pH of 2.0 in the first tube, 4.0 in the second, 6.0 in the third, 8.0 in the fourth, and a 10 pH in the fifth. Next, the enzyme lactase was added in equal amounts to each test tube and allowed to sit for ten minutes white the enzyme reacted with the lactose. At the end of the ten…

1. For each reaction below, indicate in which direction the equilibrium shifts when the stated stress is applied to the system. Write NC for no change, L for left, and R for right as an indication of change in the direction of the reaction. Note: Always work with a balanced chemical equation. Stress _1. PCI5 (9) I PCI3 (9) + Cl2 (9) + heat temperature decrease 2. CO (9) + Fe3O4(s) I CO2 (g) + 3FeO(s) volume increase 3. Heat + H2 (g) + 12 (9) | 2Hl(g) temperature increase _4. N2 (g) + 3H2 (g) | 2 NH3 (g) pressure decrease 5. NO(g) + O2 (g) I N2O3 (9) concentration increase

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

Solve correctly please. (Gpt/ai wrong answer not allowed)

Write the equation for the equilibrium constant (K) of the reaction studied in this exercise. 2CrO4 2- (aq) + 2H+ (aq) = Cr₂O72- (aq) + H₂O(1) 1E T² B 1 U T₂ 0 Word(s)

please help with this question. it's not an assay, but calculation. thanks

2MnO4−+5H2C2O4+6H+⟶2Mn2++10CO2+8H2O Reaction : Permanganate Ion Reduced by Oxalic Acid If you increase the concentration of oxalic acid in an experiment, what will the molecules and ions be doing? (Simply trying to determine how it will be effected because I don't understand what it would be doing. In the experiment I did, it took longer to notice any changes occur in the color of the test I was doing. )

Nitrous acid (HNO2) is an essentially nonvolatile acid that ionizes in water with an equilibrium constant of 4 x 10-4 mol/liter. Assume that 10 mmol of nitrous acid are added to a liter of water that is open to the atmosphere.a. List all chemical species that you expect to occur in the water. For which of these do you know the concentration a priori? (you may assume the water has reached equilibrium with the air, and therefore H2CO3* concentration is approximately 12 mM, per Henry’s law)b. Write every equation that constrains the composition of the system at equilibrium identifying each as a mass conservation, mass action, or electroneutrality constraint.

. Use stoichiometry to determine the equilibrium [Fe3+] and [SCN-] in each test tube. y = 6170.7x - 0.0153 Solution  0.002M iron(III) nitrate in 1M nitric acid(mL) 0.002M potassium thiocyanate(mL) DI water(mL) Absorbance(A) 1 3 2 1 0.128 2 2 3 1 0.269

11. Given the following equilibria and equibrium constants: 1/2 N₂ (g) + 1/2 O₂ (g) NO (g) Kc = 4.8 × 10-10 2 NO₂ (g) 2 NO(g) + O₂(g) Kc = 1.1 x 10-5 | a. What is the value of Ke for the following reaction? Show your work! 2 NO₂ (g) N₂ (g) + 2 O₂ (g) Kc = b. In a container, [NO₂] = [N₂] = [0₂] = 1.000 × 10-5 M. Prove or disprove that the mixture in the container is at equilibrium. If the mixture is not at equilibrium, explain which species will change concentration, and how those concentrations will change.

Use the systematic treatment of equilibrium to calculate the concentration of Ba2+ in acidic solution, if its concentration is governed by the following equilibria - BaSO4(s) → Ba2+ + SO2-4 Ksp = 1.1 x 10-10 SO2-4 +H2O → HSO-4 +OH- Kb = 9.8 x 10-13 Ba2+ + SO2-4 → BaSO4(aq) Kf = 1.9 x 101 Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Use the mass balance for your calculation.

2. Which of the following statements about reaction quotient (Qc) is FALSE?                 a. The equation used is aA + bB is reversible by cC + dD                 B. It is used to determine if chemical equilibrium is                  C. If Qc < Kc, the products dominate in the chemical                  D. If chemical equilibrium is not achieved, Qc is used to determine where the direction of reaction will proceed in order to attain the 3. If the computed Kc of an unknown compound is equal to 3, where does chemical equilibrium lie?  a. center       b. left        C. right             D. left to right

Use the data provided to answer the question

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2. Is the following equilibrium reaction homogeneous or hetero- geneous? CaF₂ (s) Ca²+ (aq) + 2F- (aq) + heat 3. Write the equilibrium constant expression for the reaction CaF₂ (s) Ca²+ (aq) + 2F- (aq) + heat. 2

Write the equilibrium constant expression for the following reaction:C6H12O6(s)+6O2(g)↔6CO2(g)+6H2O(g) a. [H2O]^6 / [C6H12O6][O2]^6 b. [CO2]^6[H2O]^6 / [C6H12O6] c. ([CO2]^ 6 / [C6H12O6][O2]^6 d. None of these. e. [CO2]^6[H2O]^6 / [O2]6

4a. The solubility product for Ag3PO4: Ag3PO4(s) 3Ag+ + PO is L₁ = 8.9 × 10-17 M². The solubility product for Ag2CrO4: Ag2CrO4(s) 2Ag+ + Cro is L2 = 1.1 × 10-12 M³. Calculate, based on this, the equilibrium constant K for the following equilibrium: 3Ag2CrO4(s) + 2PO¾¼¯¯ ↔ 2Ag¸PO4(s) + 3Cro²¯¯ 4b. Calculate the concentration of Sn²+ and the pH in water shaken to equilibrium with Sn(OH)2(s). The solubility product for Sn(OH)2 is L = 5.5 × 10-27M³. The ion product of water Kw 1.0 × 10-14 M². = 4c. Calculate the concentration of Y³+ and the pH in water shaken to equilibrium with Y(OH)3(s). The solubility product for Y(OH) 3 is L = 1.0 x 10-22 M².

Please answer question 2 abc just send me the paper solutions ASAP

At equilibrium, the concentration of N2 is 5.32x10-3 M, O2 is 3.28 x10-3 M and that of NO is 6.19 x10-6 M. Evaluate the equilibrium constant for this reaction.

Determine the equilibrium constant for the following and whether it is product or reactant favored 2A +B <--> 3C the concentration of A at equilibrium is 1 M the concentration of B at equilibrium is 1 M the concentration of C at equilibrium is 3 M