Recent questions in Chemical equilibrium

0 votes

1 answer 51 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 TeresitaJack (470 points)

0 votes

1 answer 51 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 KarinLlanos6 (590 points)

0 votes

1 answer 58 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 Jacquie6021 (490 points)

0 votes

1 answer 47 views

Calculate the equilibrium constant for a reaction involving a weak oxidizing agent where the concentration of the oxidizing agent is 0.1 M and the concentration of the reduced species is 0.05 M at equilibrium. The balanced chemical equation of the reaction is given as follows:OX + 2 e- ⇌ REDwhere OX is the weak oxidizing agent and RED is the reduced species.

asked Jan 23 in Chemical equilibrium by GraceL779167 (450 points)

0 votes

1 answer 49 views

Calculate the equilibrium constant at 25°C for the reaction: CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) If at equilibrium, the concentration of CO is 0.10 M, H2 is 0.20 M, CH4 is 0.015 M and H2O is 0.035 M.

asked Jan 23 in Chemical equilibrium by TedHallstrom (470 points)

0 votes

1 answer 54 views

Calculate the equilibrium constant (Kc) of the reaction below at 25°C with and without a catalyst and determine the effect of the catalyst on the equilibrium position.N2(g) + 3H2(g) ⇄ 2NH3(g)

asked Jan 23 in Chemical equilibrium by HassieCooch5 (550 points)

0 votes

1 answer 38 views

Calculate the equilibrium constant (Kc) for the reaction between iodine (I2) and potassium iodide (KI) in an aqueous solution, given that at equilibrium, the concentration of iodine is 0.008 M and the concentration of potassium iodide is 0.15 M. The balanced equation for the reaction is given below:I2 (aq) + 2KI (aq) ⇌ 2K+ (aq) + 2I- (aq)

asked Jan 23 in Chemical equilibrium by MattieShiels (230 points)

0 votes

1 answer 53 views

Calculate the equilibrium constant (Kc) for the following reaction at 300 K: N2(g) + 3 H2(g) ↔ 2 NH3(g) given that at equilibrium, the concentration of N2 is 0.12 M, H2 is 0.20 M, and NH3 is 0.16 M.

asked Jan 23 in Chemical equilibrium by SuzanneDewee (370 points)

0 votes

1 answer 49 views

Calculate the equilibrium constant (Kc) for the following gas-phase reaction at 298 K: N2(g) + O2(g) ⇌ 2NO(g) where the initial concentrations of N2, O2, and NO are 0.100 M, 0.050 M, and 0.000 M respectively.

asked Jan 23 in Chemical equilibrium by MargretSuggs (310 points)

0 votes

1 answer 39 views

Calculate the equilibrium constant (Kc) at 25°C for the following redox reaction involving a weak oxidizing agent: H2O2(aq) + 2I^-(aq) + 2H^+(aq) ⇌ I2(aq) + 2H2O(l)

asked Jan 23 in Chemical equilibrium by MayraBeckwit (470 points)

0 votes

1 answer 57 views

Calculate the equilibrium constant (K) for the formation of the complex ion [Fe(SCN)₂⁺] when 3.0 x 10⁻³ moles of Fe(NO₃)₃ and 1.5 x 10⁻³ moles of NaSCN are mixed in a 250 mL solution. The solution shows that the concentration of Fe(SCN)₂⁺ is 1.2 x 10⁻³ M at equilibrium.

asked Jan 23 in Chemical equilibrium by Michal88L640 (770 points)

0 votes

1 answer 52 views

Calculate the equilibrium constant (K$\textsubscript{a}$) for the reaction of acetic acid in aqueous solution if the pH of the solution is 4.76 and the concentration of acetic acid is 0.1 M.

asked Jan 23 in Chemical equilibrium by FlynnChriste (210 points)

0 votes

1 answer 50 views

Calculate the equilibrium concentrations of reactants and products for the following reaction at a temperature of 25°C and a pressure of 1 atm:2 NO(g) + Br2(g) ⇌ 2 NOBr(g)Given the initial concentrations are [NO] = 0.20 M, [Br2] = 0.35 M, and [NOBr] = 0.015 M. The equilibrium constant (Kc) for the reaction is 4.8 x 10^2 at 25°C.

asked Jan 23 in Chemical equilibrium by KathieVoyles (470 points)

0 votes

1 answer 40 views

Calculate the equilibrium concentration of each species (in mol/L) in a system containing 0.200 M KI and 0.200 M Cl2 that forms KCl and I2 at equilibrium, given that the equilibrium constant (Kc) is 9.0 x 10^-2 at a certain temperature.

asked Jan 23 in Chemical equilibrium by BXXGarry4657 (270 points)

0 votes

1 answer 46 views

Calculate the effect of adding a catalyst on the equilibrium position of the following redox reaction: Fe2+(aq) + H2O2(aq) + 2H+(aq) ⇌ Fe3+(aq) + 2H2O(l) If a catalyst is added to the reaction mixture, what will be the new equilibrium constant (Kc)? And how will the addition of a catalyst affect the value of Kc?

asked Jan 23 in Chemical equilibrium by ManualSweene (470 points)

0 votes

1 answer 33 views

Calculate the effect of adding a buffer solution consisting of equal amounts of acetic acid (pKa = 4.76) and sodium acetate to a 0.1 M solution of acetic acid (Ka = 1.8 x 10^-5) at equilibrium. The volume of the buffer added is equal to the volume of the acetic acid solution.

asked Jan 23 in Chemical equilibrium by MonaHolloway (330 points)

0 votes

1 answer 44 views

At room temperature, the equilibrium constant (K) for the formation of a complex ion is 8.0 x 10^-5. If the temperature is increased by 10 degrees Celsius, how will the equilibrium constant be affected? Provide a numerical answer and explanation to support your reasoning.

asked Jan 22 in Chemical equilibrium by EstelleDibel (790 points)

0 votes

1 answer 57 views

Assuming you have the equilibrium constant value for a given chemical equation, determine the concentration of products and reactants at equilibrium for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g); Kc = 6.0 x 10^2 at 500°C. If the initial concentration of N2 is 0.1 M and the initial concentration of H2 is 0.2 M, what is the concentration of NH3 at equilibrium?

asked Jan 22 in Chemical equilibrium by AntoinetteHo (430 points)

0 votes

1 answer 40 views

Assuming the volume of a container at equilibrium is 2 L, what is the new equilibrium concentration of NOCl if the volume is changed to 1 L, given that the initial concentration of NOCl is 0.10 M and the equilibrium constant (Kc) is 0.054?

asked Jan 22 in Chemical equilibrium by TajCountryma (290 points)

0 votes

1 answer 49 views

Assuming that the volume of the system is constant, how will the equilibrium concentration of reactants and products be affected if the temperature is increased for the following reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) (a) Predict the direction of the reaction shift and explain why(b) Predict the effect of the temperature change on the equilibrium value of Kc for the reaction.

asked Jan 22 in Chemical equilibrium by BrigetteFinc (510 points)

Recent questions in Chemical equilibrium

Categories