Recent questions in Chemical equilibrium

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What is the effect of adding a catalyst on the equilibrium position of a redox reaction where iodate ions combine with sulfite ions in an acidic solution to create iodide ions and sulfate ions? Calculate the new equilibrium constant with and without the catalyst given the reaction equation: IO3^- (aq) + 3SO3^2- (aq) + H2O (l) → I^- (aq) + 3SO4^2- (aq) + 2H+ (aq) Assume the temperature, pressure and volume remain constant, and that the initial concentrations of each reactant and product are known.

asked 5 days ago in Chemical equilibrium by AnjaDacomb65 (410 points)

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1 answer 43 views

What is the effect of adding a catalyst on the equilibrium position of a redox reaction between potassium permanganate and oxalic acid if the reaction has already reached equilibrium at a specific temperature and pressure? Provide a detailed explanation and show your calculations.

asked 5 days ago in Chemical equilibrium by EttaYokoyama (710 points)

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1 answer 49 views

What will be the effect of adding a buffer solution on the equilibrium constant of an acid-base reaction between a weak acid and its conjugate base? Provide a step-by-step calculation showing the change in equilibrium position and the final pH value after the addition of the buffer solution.

asked 5 days ago in Chemical equilibrium by AnibalForman (510 points)

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1 answer 42 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 6 days ago in Chemical equilibrium by RileyLort122 (830 points)

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1 answer 46 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 6 days ago in Chemical equilibrium by JaninaBurgin (310 points)

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1 answer 78 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 6 days ago in Chemical equilibrium by GuyHnw491160 (670 points)

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1 answer 64 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 6 days ago in Chemical equilibrium by JacelynElsey (370 points)

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1 answer 52 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 6 days ago in Chemical equilibrium by CasimiraCuri (770 points)

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1 answer 36 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 6 days ago in Chemical equilibrium by HSRZak712052 (690 points)

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1 answer 63 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 6 days ago in Chemical equilibrium by AlicaOjeda8 (430 points)

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1 answer 43 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 6 days ago in Chemical equilibrium by KathrinDesco (370 points)

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1 answer 57 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 6 days ago in Chemical equilibrium by WadeCiy8478 (550 points)

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1 answer 66 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 6 days ago in Chemical equilibrium by TammyChapdel (250 points)

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1 answer 36 views

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

asked 6 days ago in Chemical equilibrium by ChanaMedwort (270 points)

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1 answer 5 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 6 days ago in Chemical equilibrium by KandiDempste (430 points)

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1 answer 33 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 6 days ago in Chemical equilibrium by OtisAlbarran (590 points)

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1 answer 36 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 6 days ago in Chemical equilibrium by AngelineFlin (510 points)

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1 answer 53 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 ImaSchardt52 (390 points)

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1 answer 48 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 HamishChappe (530 points)

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1 answer 9 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 ElmerAnderse (470 points)

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