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- 7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.Hemoglobin (Hb) and oxygen gas form a complex (HbO2) that carries oxygen throughoutthe human body. Unfortunately, carbon monoxide binds to hemoglobin so strongly that itdisplaces the oxygen already bonded there by the below equilibrium reaction:HbO2 + CO ⇌ HbCO + O2Thus, CO is toxic by reducing the concentration of HbO2 in the blood. Using the principles ofequilibrium, explain how the following first aid treatments for carbon monoxide poisoning mighthelp restore the HbO2 concentration.a. Removing the victim to an area with a safe (lower) amount of CO.b. Administering oxygen.At T = 500◦C, Kc = 169 for the gas-phasereactionA + B ⇀↽ C + DStarting with 3.64 moles each of A and B ina 5.00 liter container, what will be the equilibrium concentration of C at this temperature?Answer in units of M.
- Given that the Ka for HOCl is 3.5 10-8, calculate the K value for the reaction of HOClwith OH- at 25oC.Hello, I'm working on equilibriums, I'm not quite sure how to do this type of question with finding how much to raise a certain ammount. Any help is appreciated, thanks! CO(g) + H2O(g) ↔ CO2(g) + H2(g) is at equilibrium with concentrations as follows: [CO(g)] = 0.30 mol/L, [H2O(g)] = 0.10 mol/L,[CO2(g)] = 0.20 mol/L and [H2(g)] = 0.60 mol/L. What concentration of H2O(g) must be forcedinto the system to raise H2(g) to 0.70 mol/L?In the reaction 450.0⁰c: caco3(s) ⇌ cao(s) + co2(g), at equilibrium, if pco2 = 0.0160 atm , what is the value of Kc
- Equilibrium constant of borneol isomerization (C10H17OH) to isoborneol,in the gas phase at a temperature of 503 K is 0.106. 5.0 L flaskcontaining 7.50 g of borneol and 14.0 g of isoborneol was heated to 503 K iallowed to stabilize. Calculate the mole fractions of both components wstate of equilibriumThe following system was set up and allowed to come to equilibrium: 2 NO2(g) ⇌ N2O4 At equilibrium, the concentration of nitrogen dioxide was 2.45 mol/L, and the value of the equilibrium constant for the reaction at that temperature is 0.835. What was the concentration of the dinitrogen tetraoxide? Answer in mol/L to 3 decimal places.The equilibrium at 25 °C MaCl5 (aq) + 4 H2O (l) ↔ H3MaO4 (aq) + 5 HCl (aq) Kc = 5500 ΔH°(rxn) = 28.1 kJ/mol, Determine the ΔG°(rxn)
- Consider the reaction HOCl + F– HF + OCl– Given that K a for HOCl is 3.5 × 10 –8 and the K a for HF is 7.2 × 10 –4 (both at 25°C), which of the following is true concerning K for the above reaction at 25°C? a. K is greater than 1b. K is less than 1c. K is equal to 1d. Cannot be determined with the above informatione. none of theseconsider the folllowing reaction at equilibrium. what effect will increasin gthe temp have on the system? see both imagesIf Kc = 1 for the equilibrium 2 A(g) ⇌ B(g), what isthe relationship between [A] and [B] at equilibrium?