Learning Goal:To understand how to calculate the equilibrium constants for chemical equations that can be produced by the addition of other chemicalequations with known equilibrium constants.For a chemical reaction equation with the general formthe equilibrium equation is given byThus, for a chemical reaction equation with the general formthe equilibrium equation is given byIf the first two equations are added together such thatthen the equilibrium equation is given byorK3aA + bB =cC + dD=K₁ =cC + dD=eE+fFK2 =[C] [D]d[A]ª[B]b[E] [F][C]c[D]daA +bB=eE+fF=[E] [F] [CD][A]a[B]b [A]a[B][E] [F][C]c[D]dK3 = K₁ K₂Thus, when a chemical equation is the sum of two chemical equations for which equilibrium constants are already known, the equilibriumconstant for the reaction is the product of the equilibrium constants for the individual reactions. Keep in mind that equilibrium equations do notinclude expressions for any pure solids or liquids that may be involved in the reaction. ▼ Part AGiven the two reactions1. H₂S(aq) = HS(aq) + H+ (aq),K₁=9.82x108, and2. HS (aq) = S2 (aq) + H+ (aq),K₂ = 1.56x10-19,what is the equilibrium constant Kfinal for the following reaction?Enter your answer numerically.► View Available Hint(s)Kfinal = 6.53x1025Submit✓ Correct▾ Part BPrevious AnswersGiven the two reactions3. PbCl2 (aq) = Pb²+ (aq) + 2Cl(aq), K3=1.79x10-10, and4. AgCl(aq)Ag+ (aq) + Cl(aq),K₁=1.15x10-4,what is the equilibrium constant Kfinal for the following reaction?Express your answer numerically.► View Available Hint(s)Submit| ΑΣΦΠΠKfinal 1.32-10-²Previous AnswersX Incorrect; Try Again; 5 attempts remaining?S² (aq) + 2H+ (aq) = H₂S(aq)PbCl₂ (aq) + 2Ag+ (aq) = 2AgCl(aq) + Pb²+ (aq)

Answered: Image /qna-images/answer/a9de38ab-bbbf-4d44-aaf8-03460ab871a1.jpg

Part A Given the two reactions 1. H₂S(aq) HS (aq) + H+ (aq), K₁=9.82x10-8, and 2. HS (aq) = S²(aq) + H+ (aq), K₂ = 1.56x10-19, what is the equilibrium constant Kfinal for the following reaction? Enter your answer numerically. ► View Available Hint(s) Kfinal 6.53x1025 Submit Previous Answers ✓ Correct Part B Given the two reactions 3. PbCl2 (aq) = Pb²+ (aq) + 2Cl(aq), K3=1.79x10-10, and 4. AgCl(aq) Ag+ (aq) + Cl(aq), K4 = 1.15x10-4, what is the equilibrium constant Kfinal for the following reaction? Express your answer numerically. ► View Available Hint(s) ΕΠΤΑΣΦ Kfinal=1.32 10-² Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining ? S² (aq) + 2H+ (aq) = H₂S(aq) PbCl₂ (aq) + 2Ag+ (aq) = 2AgCl(aq) + Pb²+ (aq)

Part A Given the two reactions 1. H₂S(aq) HS (aq) + H+ (aq), K₁=9.82x10-8, and 2. HS (aq) = S²(aq) + H+ (aq), K₂ = 1.56x10-19, what is the equilibrium constant Kfinal for the following reaction? Enter your answer numerically. ► View Available Hint(s) Kfinal 6.53x1025 Submit Previous Answers ✓ Correct Part B Given the two reactions 3. PbCl2 (aq) = Pb²+ (aq) + 2Cl(aq), K3=1.79x10-10, and 4. AgCl(aq) Ag+ (aq) + Cl(aq), K4 = 1.15x10-4, what is the equilibrium constant Kfinal for the following reaction? Express your answer numerically. ► View Available Hint(s) ΕΠΤΑΣΦ Kfinal=1.32 10-² Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining ? S² (aq) + 2H+ (aq) = H₂S(aq) PbCl₂ (aq) + 2Ag+ (aq) = 2AgCl(aq) + Pb²+ (aq)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Solve questions 2-10, thanks. 1 HgO(s) + 2 I−(aq) + H2O(l) ⇄ HgI2(g) + 2 OH−(aq) ; ∆H < 0 Consider the equilibrium above. Which of the following changes will increase the concentration of HgI2? (A) Increasing the concentration of OH− (B) decreasing the pressure (C) Increasing the mass of HgO present (D) Increasing the temperature (E) Adding a catalyst 2 In which of the following systems would the equilibrium NOT be shifted by a change in the volume of the system at constant temperature? (A) CO(g) + NO(g) ⇄ CO2(g) + 1/2 N2(g) (B) N2(g) + 3 H2(g) ⇄ 2 NH3(g) (C) N2(g) + 2 O2(g) ⇄ 2 NO2(g) (D) N2O4(g) ⇄ 2 NO2(g) (E) NO(g) + O3(g) ⇄ NO2(g) + O2(g) 3. What substance is missing in the following reaction mechanism? Step 1 NO + ___ à OONO Step 2 NO + OONO à 2NO2…
Give detailed Solution with explanation needed (don't give Handwritten answer
Question 37 of 51 Submit Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 x 10-4 at a certain temperature. If a solid sample of CaCro. dissolves in solution, what will the equilibrium concentration of Ca" in the solution be? CaCro-(s) = Ca"(aq) + Cro. (aq) NEXT> 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. Cacro.(s) = Ca* (aq) + Cro.(aq) Initial (M) |Change (M)upriu Equilibriu m (M). RESET 7.1 x 10- +2x -2x 7.1 x 10+x 7.1 x 10-x 7.1 x 10+ 2x 7.1 x 10-2x +
WRITE THE EQUILIBRIUM EXPRESSIONS FOR EACH OF THE FOLLOWING: (A) CO(G) + 2H2(G) <- -> CH3OH(G) (B) 2NO2 (G) <- -> 2NO(G) + O2(G) (C) P4 (G) + 6 BR2 (G) <- -> 4 PBR3(G)
he following equilibrium constants at 427°C: +4Na(1) 2Na2O(s) K₁ = 2.50x1049 +2Na(1) 2NaO(g) K₂ = 2.50x109 +2Na(1) Na2O2(s) K3 = 2.00×1028 + Na(1) NaO₂(s) K4 = 3.33×1013 ould be the value of the equilibrium constant for each of the following reactions, at 427°C? +2Na2O2(s) 2NaO(g) + 2NaO2(s) -12 Answer Incorrect. Tries 3/8 Previous Tries (s) +Na() 2NaO(g) 26 Answer Incorrect. Tries 1/8 Previous Tries
Consider the following equilibrium for nitrous acid, HNO2 a weak acid: HNO2 (aq) + H2O (l) H30' (aq) + NO2(aq) ΔΗ > O 麷 m In which direction ( shift, if: -a) NaOH is added? Left, Right or No effect will the equilibrium Select l - b) NaNO2 is added? I Select ] c) HCI is added? I Select ] d) The acid solution is made more dilute? l Select Next
Consider the following system at equilibrium where AH° = 268 kJ, and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) → NH3 (g) + HCl(9) When some moles of NH4Cl(s) are removed from the equilibrium system at constant temperature: The value of Ke Oincreases decreases Oremains the same The value of Qc Ois greater than Ke Ois equal to Ke Ois less than Kc The reaction must run in the forward direction to reestablish equilibrium. run in the reverse direction to reestablish equilibrium. remain the same. It is already at equilibrium. The number of moles of NH3 will Oincrease decrease Oremain the same
Write equilibrium constant (K) expressions for the following reactions: 1. a. HF (aq) H20 (1) F- (aq) H30+ (aq)
QUESTION 1 Consider the following equilibrium reaction. CO2(g) + 2H2(g) СН3ОН(g) ДНО %3 -90.8 kJ Which of the following will increase the equilibrium constant, K? а. Increase in temperature. b. ·Increase in amount of CH3OH(g). С. Increase in pressure. d. Decrease in pressure. е. Decrease in temperature. QUESTION 2 The anion of a weak acid а. will produce H+ ions in water. b. is an acidic ion. С. is a basic ion. d. is a neutral ion. е. will lower the pH of the solution.
A (aq) + 2 B (g) ⇌ C (aq) + 2 D (aq) + heat (a) How will the above reaction shift when the concentration of A is increased? (left, right, no shift) (b) D forms F when reacted with E. How will the above reaction shift when E is added? (left, right, no shift) (c) What temperature and pressure will maximize the yield of product? Temperature: (high, low, no affect) Pressure: (high, low, no affect)
4NH3(g) +302(g) = 2N2(g) +6H20(g) The initit concentrations of NH3 and 02 are both 0.021 Mat a certain temp. Once system reaches equilibrium, the N2 concetration is determined to be 0.00449, what is the equilibrium constant. of 02? (3 sig fig normal notation
> Given the two reactions HS (aq) +H (aq), K₁=9.70x108, and 1 1. H₂S(aq) 2. HS (aq) S² (aq) +H(aq), K₂=1.55x10-19, what is the equilibrium constant Kfinal for the following reaction? Enter your answer numerically. ▸View Available Hint(s) 1D ΑΣΦΑ Kfinal 1.078 1026 Submit ● Part R Previous Answers S² (aq) + 2H* (aq) = H₂S(aq) X Incorrect; Try Again; 9 attempts remaining ?