Recent questions in Chemical equilibrium

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Consider the chemical reaction A(g) + B(g) ↔ 2C(g). At equilibrium, the concentration of A is 0.25 M, the concentration of B is 0.15 M, and the concentration of C is 0.40 M. What is the equilibrium constant for this reaction at the given temperature?

asked Feb 3 in Chemical equilibrium by ChastityHoll (1.8k points)

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1 answer 37 views

Consider a weak acid, HA, with a dissociation constant, Ka = 1.8 x 10^-5. What will be the effect on the concentration of [H3O+] and the degree of ionization of the acid if 0.1 moles of HCl is added to 1 liter of a 0.1 M solution of HA?

asked Feb 3 in Chemical equilibrium by RafaelaBabb7 (2.0k points)

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Consider a chemical reaction in which X and Y combine to form XY at equilibrium: X + Y ⇌ XY The equilibrium constant for the reaction is Kc = 1.2x10^-4. Initially, [X] = 0.2 M and [Y] is unknown. If 0.1 M of Y is added to the reaction mixture, what will be the new equilibrium concentration of XY?

asked Feb 3 in Chemical equilibrium by LeeAlder0448 (1.5k points)

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1 answer 69 views

Calculate the percentage change in the concentration of reactants and products in a chemical equilibrium when the concentration of a common ion is increased by 0.1M. The equilibrium constant for the reaction is Kc = 1.5 x 10^-5 M at a certain temperature.

asked Feb 3 in Chemical equilibrium by DarylBottoml (2.0k points)

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1 answer 59 views

Calculate the new equilibrium concentration of a complex ion formed between Cu2+ and NH3(aq) at 25°C, if the initial concentration of Cu2+ is 0.10 M and NH3(aq) is 0.05 M, and the temperature is increased to 35°C. The equilibrium constant (Kc) for this reaction is 1.6×107.

asked Feb 3 in Chemical equilibrium by JanF74978399 (1.6k points)

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1 answer 82 views

How does changing the volume affect the equilibrium position of a chemical reaction? Provide an example of a reaction and calculate the new equilibrium concentrations when the volume is decreased by a certain factor.

asked Feb 3 in Chemical equilibrium by VioletteM27 (2.1k points)

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1 answer 110 views

How does changing the temperature affect the equilibrium constant (Kc) and the formation of Fe(SCN)2+ complex ion from Fe3+ and SCN- ions?

asked Feb 3 in Chemical equilibrium by AltonDurden (2.1k points)

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1 answer 57 views

How does changing the pH affect the equilibrium position of the redox reaction: Fe2+ + 2H+ ⇌ Fe3+ + H2O?

asked Feb 3 in Chemical equilibrium by Agustin3989 (1.7k points)

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1 answer 66 views

How will changing the pH affect the formation of a complex ion between Fe³⁺ and CN⁻ in a solution containing both species at equilibrium? Provide a theoretical explanation supported by relevant chemical equations and calculations.

asked Feb 3 in Chemical equilibrium by NinaDimattia (1.6k points)

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1 answer 61 views

How does changing the pH affect the formation of a complex ion with copper (II) ion and ethylenediamine? Provide a detailed explanation and the associated chemical equations.

asked Feb 3 in Chemical equilibrium by Lionel426684 (2.1k points)

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1 answer 63 views

How does changing the pH of a solution affect the equilibrium position of an acid-base reaction between a weak acid and its conjugate base? Provide a detailed explanation and real-life examples.

asked Feb 3 in Chemical equilibrium by ElviaBumgarn (1.8k points)

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1 answer 62 views

How does changing the pH of a solution affect the formation of a complex ion using the example of [Cu(H2O)6]2+ forming [Cu(NH3)4(H2O)2]2+ at different pH values? Provide an explanation based on Le Chatelier's principle.

asked Feb 3 in Chemical equilibrium by RemonaRainey (1.6k points)

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1 answer 81 views

How does changing the pH of a solution affect the equilibrium position of a weak acid-base reaction? Provide an example to support your answer.

asked Feb 3 in Chemical equilibrium by KaylaTibbett (1.9k points)

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1 answer 62 views

How does changing the pH affect the equilibrium position of a redox reaction involving a weak acid and its conjugate base? Provide a specific example to illustrate your answer.

asked Feb 3 in Chemical equilibrium by JoelPrentice (1.4k points)

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1 answer 60 views

How does changing the pH of a solution affect the equilibrium position of a redox reaction between copper and silver ions? Provide a detailed explanation with chemical equations and the relevant equilibrium constants.

asked Feb 3 in Chemical equilibrium by OrenTherrien (1.8k points)

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1 answer 65 views

How does changing the pH affect the equilibrium constant (Kf) for the formation of Fe(CN)6 4- complex ion in a solution containing Fe3+ and CN- ions? Provide a detailed explanation of the effect of pH on the equilibrium constant for the reaction.

asked Feb 3 in Chemical equilibrium by NelleVxq8414 (1.5k points)

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1 answer 51 views

How does changing the pH of a solution affect the equilibrium position of an acid-base reaction when starting with HF (hydrofluoric acid) and NaOH (sodium hydroxide)?

asked Feb 3 in Chemical equilibrium by TrudiMarron (1.6k points)

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1 answer 47 views

How does changing the pH of a solution affect the equilibrium position of an acid-base reaction, and what factors influence this effect? Provide examples of acid-base equilibria and their changes in equilibrium position with changes in pH.

asked Feb 3 in Chemical equilibrium by LeifLeverett (2.3k points)

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1 answer 86 views

How does changing the pH affect the equilibrium position of an acid-base reaction between a weak acid and a strong base? Provide a brief explanation of the underlying principle and use an example to illustrate your answer.

asked Feb 3 in Chemical equilibrium by WPOBernadine (1.9k points)

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1 answer 105 views

How does changing the pH of a redox reaction involving Fe3+ and Fe2+ affect the equilibrium position of the reaction, and how can this be predicted using the Nernst equation?

asked Feb 3 in Chemical equilibrium by StefanHartin (1.7k points)

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