Scoring: Your score will be based on the number of correct matches minus the number of incorrect matches. There is no penalty for missing matches.Use the References to access important values if needed for this question.For the following reaction, the reactants are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids orbases.F + C6H5NH3+ ⇒HF + C6H5NH2HFClear AllStronger Bronsted-Lowry acidWeaker Bronsted-LowryC6H5NH3+acidF-Stronger Bronsted-Lowry baseC6H5NH2Weaker Bronsted-Lowrybase

Step 1:Backward reaction is spontaneous reaction HF - proton donar, strong acid F- - proton…

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Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 17STP

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Describe any thermochemical (heat of reaction) evidence for the Arrhenius concept.
What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) HCIO4 + H2O (b) NH4 ++ H2O (c) HCO3 + OH
Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
. a. Write the conjugate acid for each of the following Brønsted-Lowry bases. NO3.HSO4,ClO4,NH3,HCO3b. Write the conjugate base for each of the following Brønsted- Lowry acids. HCI,H2SO4,NH3,NH4,HCO3
For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. HCOOH + C3H]N=HC00 + C3H]NH* Clear All C3H]NH Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry HCOO acid Stronger Bronsted-Lowry base C3H]N Weaker Bronsted-Lowry HCOOH base Previous Next
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species prese equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCH, CO, is a weak acid. 1.3 mol of KOH is added to 1.0 L of a 1.3M HCH,CO₂ solution. 0.2 mol of HNO3 is added to 1.0 L of a solution that is 0.5M in both HCH3CO₂ and NaCH, CO₂. acids: ☐ bases: ☐ X 5 O other: ☐ acids: ☐ ☐ bases: ☐ ☐ other: ☐
Pick the statement that best describes a reversible reaction when reactants are first mixed together. The rate of the forward reaction is faster than the rate of the reverse reaction. The rate of the forward reaction is slower than the rate of the reverse reaction. The concentration of reactants is lower than the concentration of products. The reaction is at equilibrium from the start.
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Hi, I only need help with question # 3. Equilibrium Write the equilibrium expressions for the following reactions:a) 3Fe(s) + 4H2O(g) ↔ Fe3O4(s) + 4H2(g)b) CH3COOH(aq) + H2O(l) ↔ CH3COO-(aq) + H3O+(aq)c) N2(g) + 3Br2(g) ↔ 2NBr3(s)d) CaCl2(s) ↔ Ca2+(aq) + 2Cl-(aq) Consider the following equilibrium: CH3COOH(l) + C2H5OH(l) ↔ CH3CO2C2H5(l) + H2O(l) Keq =2.2 What must the concentration of water be for a mixture with [CH3COOH]= 0.10M, [CH3CO2C2H5]=2.0M, [C2H5OH]= 5.0M to be at equilibrium? Note: water is NOT the solvent in this reaction, therefore it will be included in the equilibrium expression. 3. Predict the direction of the following equilibrium shifts (Please label Forward (F) or Reverse (R)): a) H2O (g) + CO(g)↔ H2(g) + CO2(g) Water is removed? ___Hydrogen is added? ___Carbon monoxide is added? ___b) 4Fe(s) + 3O2(g) ↔ 2Fe2O3(s) + 1648 kJThe temperature is increased? ___The pressure is increased? ___c) CaCl2(aq) ↔ Ca2+(aq) + 2Cl-(aq) NaCl is added? ___AgNO3 is added? ___
Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5. Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.
Use Le Châtelier's Principle to determine in which direction equilibrium will shift in each scenario. Complete the following charts by writing left, right, or none for the equilibrium shift, and decreases, increases, or remains the same for the concentrations of reactants and products. [A, 12:4 each problem set] Evaluation Rubric 1. Using Le Chatelier's Principle, predict whether the equilibrium shifts towards the reactants (left), or towards the products (right), or will have no shift, given the following conditions. Justify your reasoning. Nz(g) + 3H2(g) > 2NH3(g) + 22.0 kcal (heat) ww Stress Equilibrium Reasoning Shift Add N2 Remove H2 Increase Temperature Increase Pressure +
Which expression shows a reversible reaction at equilibrium? O AH>0 Ο ΔΗ AH = 0 O AS>0 O AS 0

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