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4. Consider the following equilibrium system. CO2(aq) + 2 F-(aq) + H2O(1) = CO32-(aq) + 2...
Identify the conjugate acid-base pairs in each of the following equations: 1) HF(aq)+CO32?(aq)?F?(aq)+HCO3?(aq) Check all that apply. a) F?/HCO3? b) HF/F? c) HF/CO32? d) HCO3?/CO32? 2) HCl(aq)+OH?(aq)?Cl?(aq)+H2O(l) a) HCl/OH? b) HCl/Cl? c) H2O/OH? d) H2O/Cl?
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0580 M, [H2] = 0.0430 M, [CO2] = 0.0830 M, and [H2O] = 0.0370 M. (a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.460 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: M CO: M...
Consider the following equilibrium process at 686 ° C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0880 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686 ° C. (b) If we add CO2 to increase its concentration to 0.510 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M...
Consider the following equilibrium reaction: CaCO3 (s) + CO2 (g) + H2O (l) ⇌ 2 HCO3- (aq) + Ca2+ (aq) Which of these species should be included in the equilibrium constant expression (K) for this reaction? Select all that apply A.) Ca2+ (aq) B.) CaCO3 (s) C.) H2O (l) D.) CO2 (g) E.) HCO3- (aq)
e chemical equation for the dissociation of HCIO2 in water is: HClO2(aq) = H(aq) + CO2(aq) K = 1.1 X 10-2 are the equilibrium concentrations of HClO2(aq) and CO2 (aq), and the pH of a 0.1 M solution? a. 0.064 M, 0.036 M and 1.19 b. 0.072M, 0.028 M and 1.55 c. 0.067M, 0.032 M and 1.50 d. 0.072 M, 0.028 M and 1.14 e. 0.067 M, 0.033 M and 1.48
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...
estion 10 of 65 > Consider the reaction. HF(aq) + KOH(aq) — KF(aq) + H20(1) What is the net ionic equation for the chemical reaction? HF(aq) + K+(aq) + OH(aq) — K+(aq) + F (aq) + H2O(1) O HF(aq) + K+(aq) + OH-(aq) — K+(aq) + F (aq) + H+(1) + OH-(1) O HF(aq) + OH-(aq) —> F-(aq) + H2O(1) HF(aq) + K+(aq) F (aq) + H+(1) HF(aq) + K+(aq) K+(aq) + H2O(1) - 11 of 65 > Calculate either...
Atmospheric CO2 (g) is in equilibrium with dissolved CO, (aq), CO2(g) CO2 (aq) CO: (aq) then can react with water to become H_CO. CO2 (aq) + H:0 (1) ~ HCO, (aq) (2) Add the two reactions together and determine the overall net reaction. If the K, for reaction (1) is 1.44 x 10-4 and for reaction (2) the K is 1.90 x 10-2, then what would the K, for the overall net reaction be? Explain. Increasing CO, (g) would have...
1. Write the equilibrium constant expression for the following reaction: H3PO4(aq) + 3 H2O(l) ↔ PO4 3- (aq) + 3 H3O+ (aq) 2. (LeChatlier’s principle) The following reaction has Kc = 4.2 x 102 at 325oC, all gases. PBr3 + Cl2 ↔ PCl3 + Br2 ΔHo = -47 kJ/mol a. For this reaction at equilibrium, [PBr3] = [Cl2] = 0.0273 M, and [PCl3] = [Br2] = 0.560 M. What do you expect to happen to the equilibrium concentrations of each...
Identify the chemical species in the carbonate system, and explain the significance of the system. Hence, on the bases of the following equilibria, determine the concentrations carbonate system species in a stream with a pH of 5.8. CO2(g) ↔ CO2(aq) KH = 3.4 x 10-2 mol L-1 atm-1; CO2(aq) + H2O ↔ H2CO3; Kr = 2 x 10-3 mol L-1 atm-1; H2CO3(aq) ↔ H+ + HCO3-; Ka1 = 4.47 x 10-7 M. HCO3- ↔ H+ + CO32-; Ka2 = 4.68...