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- Examine the following reaction. 3 CO 2 (g) + 2 Fe(s) Fe2O3(s) + 3 CO(g) What is the equilibrium expression for the reaction? O K₂= [CO]/[CO₂] OK₂ = [Fe] [CO₂]/([Fe2O3] [CO]) [Fe]/[Fe₂O3] O Kc = O Kc = [Fe]² [CO₂]³/([Fe₂O3] [CO]³) O Kc = [Fe₂O3] [CO] / [[Fe] [CO₂]) O K₂= [CO]³/[CO₂]³ OK₂ = [Fe₂O3] [CO]³/([Fe]² [CO₂]³) O Kc = [CO₂]³/[CO]³ O Kc = [Fe₂O3] / [Fe] O K = [CO₂]/[CO]Given the equilibrium expression below, the most likely equation for the reaction is: [N₂][0₂] Keq = [NOP O2NO(g) N₂(g) + O₂(g) O2NO(1) N₂(g) + O₂(g) ON2(g) + O2(g) → 2NO(1) ON2(g) + O2(g) → 2NO(g)The equilibrium between carbon dioxide gas and carbonic acid is very important in biology and environmental science. CO2 (aq) + H2O (l) H2CO3 (aq) What would be the equilibrium constant expression (Kc) for this reaction?
- Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O₂(g) 2 HgO(s) At a certain temperature, a chemist finds that a 6.4 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound Hg sequilibrium composition amount 12.2 g K₂= Writing th 0₂ 23.8 g HgO 21.5 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits.For the steam hydrocarbon reforming process, the equilibrium law expression is [CO₂(g)][H₂(g)]* [CH][H₂0² Kc The reaction described by this equilibrium is CH4 (a) + H₂O(g) = CO₂(g) + H₂(g) CH4 (q) + 2H₂O(g) = CO₂(g) + 4H₂(g) CO₂(g) + 4H₂(g) = CH₁ (a) +2H₂O(g) CO₂(g) + H₂ (a) CH4 (q) + H₂O(g)What is the the average Kc (equilibrium constant) based on this table?
- Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N2(g) + 3H2(g) = 2NH3(g) Ton: N. x10-2 ent (O Pncca waythe chemical system would 5 the vara BI U = E T O Word(s) ------ T T; O Word(s) 5. If the concentration of the product NH3 was increased from 1.0x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B I U E T O Word(s)1. Consider the following reaction: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 A 5.0 L vessel contains 0.060 mol NO, 1.0 mol O2, and 0.80 mol NO2. Is this system at equilibrium? If the system is not at equilibrium, does the reaction proceed in the forward or reverse direction to reach equilibrium?Given the following balanced chemical reaction: CO (g) + 2 H₂ (g) = CH3OH (g). Determine the value of the equilibrium constant Ke given the following the following equilibrium concentration at room temperature. . 0.40 M CO • 0.30 M H₂ . 0.060 M CH3OH
- Please note: in this question, the double arrow is used for equilibrium arrows. Consider the following reaction: 2 SO 3(9) 02(g) + 2 SO₂ At equilibrium the following concentrations are found: [0₂] = 2.00M [SO₂] = 3.00M [SO3] = 1.00M What is the value of the equilibrium constant? 6.444 X4. Hemoglobin (Hb) and oxygen gas form a complex (HbO,) that carries oxygen throughout the human body. Unfortunately, carbon monoxide also binds to hemoglobin so that an equilibrium is established. Carbon monoxide poisoning occurs when the concentration of HbO, in the blood is reduced. HbO, + CO HBCO + O2 The first aid for a person suffering from carbon monoxide poisoning is to (1) remove them to an area of fresh air, and (2) administer oxygen. Both of these processes improve the amount of HbO, that is available for the hemoglobin to carry oxygen in the blood. Using the principles of equilibrium, explain how each of these helps to increase the HbO, concentration.2:25 1 Question 18 of 25 Submit Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 x 10³ at a certain temperature. If the equilibrium concentrations of H2 and F2 are both 0.0021 M, determine the concentration of HF at equilibrium. H2(g) + F2(g) = 2 HF(g) 1 2 If [x] represents the equilibrium concentration of HF, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms.. Ko = = 2.1 x 103 5 RESET [0] [0.0021] 2[0.0021] [x] [2x] [x]? [2x]? [0.0011] 2[0.0011] [0.0011]?