Recent questions in Chemical equilibrium

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1 answer 88 views

What is the effect of increasing pressure on the equilibrium position for the following reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) Assuming the reaction is at equilibrium, how would the concentrations of SO2, O2, and SO3 be affected by increasing the pressure of the system?

asked Jan 30 in Chemical equilibrium by JaninaDohert (2.2k points)

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1 answer 100 views

What is the predicted effect of increasing the pressure on the equilibrium position of the reaction between nitrogen and hydrogen to form ammonia, N2(g) + 3 H2(g) ⇌ 2 NH3(g), at a constant temperature and volume?

asked Jan 30 in Chemical equilibrium by Linwood6326 (2.3k points)

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1 answer 115 views

Given a chemical reaction at equilibrium, if the concentration of reactants is increased, predict the direction in which the reaction will shift to establish a new equilibrium position.

asked Jan 30 in Chemical equilibrium by DebbraCarder (2.3k points)

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1 answer 99 views

What is the effect on the equilibrium position of a reaction if we add more reactant or remove product from the reaction mixture at equilibrium, specifically for the reaction: N2(g) + 3H2(g) <=> 2NH3(g)?

asked Jan 30 in Chemical equilibrium by RogerDenning (2.4k points)

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1 answer 90 views

How would a decrease in pH affect the equilibrium position of the following acid-base reaction: HA + B ↔ A- + HB+ Assuming other conditions remain constant, predict the direction in which the equilibrium will shift and explain your reasoning.

asked Jan 30 in Chemical equilibrium by Phillipp57B1 (2.3k points)

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1 answer 73 views

How would a decrease in pH affect the equilibrium position of a redox reaction involving a metal and its corresponding metal ion, with respect to the oxidation-reduction potential? Provide an explanation for your answer.

asked Jan 30 in Chemical equilibrium by MargueriteSl (1.9k points)

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1 answer 97 views

What effect does a change in the concentration of ligands have on the formation of a complex ion in a solution of FeCl3? How does this affect the equilibrium constant of the reaction and what is the relationship between the concentration of the ligands and the stability constant of the complex ion? Calculate the equilibrium concentrations of the species involved and determine their values at different stages of the reaction. Use the given data and appropriate equations to solve the problem.

asked Jan 30 in Chemical equilibrium by VonnieMyers6 (2.1k points)

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1 answer 95 views

How does a change in pH affect the formation of complex ions in a chemical equilibrium system? Provide an explanation and relevant examples.

asked Jan 30 in Chemical equilibrium by RyderShupe77 (1.7k points)

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1 answer 106 views

How does a change in pH affect the formation of the complex ion Fe(III)-thiocyanate, and what is the equilibrium constant for this reaction at a pH of 2.5?

asked Jan 30 in Chemical equilibrium by TonyaCombs22 (1.8k points)

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1 answer 160 views

How does a change in pH affect the equilibrium position of a redox reaction between iron (III) and iodide ions, and can this effect be predicted using the Nernst equation? Provide experimental data and calculations to support your answer.

asked Jan 30 in Chemical equilibrium by PriscillaLaf (1.6k points)

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1 answer 74 views

How does a change in pH affect the equilibrium position of a reaction between a weak acid and its conjugate base?

asked Jan 30 in Chemical equilibrium by KatherineRei (1.9k points)

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1 answer 37 views

Consider the reaction: 2NOBr(g) ⇌ 2NO(g) + Br2(g)The Kc value for this reaction at a certain temperature is 0.045. A catalyst is added to the reaction mixture that increases the rate of the forward and reverse reactions to the same extent. What effect will this catalyst have on the equilibrium position of the reaction mixture? Justify your answer using calculations.

asked Jan 30 in Chemical equilibrium by GraceChaves1 (2.0k points)

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1 answer 85 views

What is the effect of a catalyst on the equilibrium position of a reaction in which there are unequal numbers of gaseous reactants and gaseous products? Use the chemical equation for the reaction, the initial concentrations of the reactants and products, and the equilibrium constant (Kc) to determine the changes in reaction rate, the equilibrium concentrations of the reactants and products, and the new value of Kc when a catalyst is introduced.

asked Jan 30 in Chemical equilibrium by HazelAvelar (1.7k points)

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1 answer 107 views

What is the effect of adding a catalyst on the equilibrium position of a redox reaction and how would you calculate the change in equilibrium concentration of products and reactants? Provide an example of a redox reaction and its equilibrium constant (Kc) value before and after the addition of a catalyst. Also, explain the role of a catalyst in shifting the equilibrium position of a reaction.

asked Jan 30 in Chemical equilibrium by RosemarieKin (1.8k points)

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1 answer 65 views

Calculate the equilibrium constant, Kc, for the reaction:2SO2(g) + O2(g) ⇌ 2SO3(g) at a temperature of 600 K, given that the initial concentrations of SO2, O2, and SO3 were 0.025 M, 0.014 M, and 0 M, respectively, and at equilibrium [SO2] = 0.015 M, [O2] = 0.008 M, and [SO3] = 0.025 M.

asked Jan 23 in Chemical equilibrium by RandellBeggs (2.0k points)

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1 answer 61 views

Calculate the equilibrium constant, Kc, for the reaction below at 25°C if the concentration of CO2 is 1.2 M, the concentration of H2 is 0.8 M and the concentration of CO is 0.6 M.CO2(g) + H2(g) ⇌ CO(g) + H2O(g)

asked Jan 23 in Chemical equilibrium by JanieCorso7 (1.9k points)

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1 answer 36 views

Calculate the equilibrium constant, Kc, at 298 K for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g) when the initial concentrations of SO2, O2, and SO3 are 0.100 M, 0.200 M, and 0.300 M, respectively.

asked Jan 23 in Chemical equilibrium by HenryCharles (2.0k points)

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1 answer 78 views

Calculate the equilibrium constant, Ka, for the dissociation of a weak acid HA with an initial concentration of 0.10 M that ionizes to form H+ and A-. At equilibrium, the concentration of H+ is found to be 1.0 x 10^-5 M and the concentration of A- is 0.09 M.

asked Jan 23 in Chemical equilibrium by Sterling80B (2.1k points)

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1 answer 60 views

Calculate the equilibrium constant for the reaction: 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) if at equilibrium the concentrations are [NOCl] = 0.050 M, [NO] = 0.030 M, and [Cl2] = 0.020 M.

asked Jan 23 in Chemical equilibrium by SNBBernd7967 (2.3k points)

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1 answer 80 views

Calculate the equilibrium constant for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g), given that the concentrations at equilibrium are [SO2] = 0.20 M, [O2] = 0.30 M and [SO3] = 0.50 M.

asked Jan 23 in Chemical equilibrium by ErickB565479 (1.8k points)

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