Consider the following equilibrium: C,H6(g) + C3H12(g) = CH4(g) + C,H14(g); Kp = 9.57 at 500 K Suppose 13.3 g each of CH4 (MW= 16), C2H6 (MW = 30), C3H12 (MW = %3D 72), and CGH14 (MW = 86) are placed in a 50.0-L reaction vessel at 500 K. What is the value of Q,?
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- The following reaction can be used to make H2 for the synthesis of ammonia from the greenhouse gases carbon dioxide and methane: CH4 (g) + CO2 (g) ⇌ 2 CO (g) + 2 H2 (g) At 1200. K, Kp = 3.548 × 106. What is the partial pressure of CH4 at equilibrium when 10.00 atm of CH4 reacts with 15.00 atm of CO2 at 1200. K? Use small x approximation and calculate the percent errorThe following synthesis reaction was conducted at 325K: A2(g) + 3B2(g) ⇌ 2AB3(g). At this temperature, KP = 5.49 x 10-6. In a 3.00L flask, 0.175atm of A2(g) and 0.410atm of B2(g) are added and allowed to reach equilibrium. Calculate the pressure of AB3(g) in the system (in atm).Find the variance (F) for the following equilibria: (i) 2 CaSO4(s) ↔ 2 CaO(s) + 2 SO2(g) + O2(g) (2) (ii) CuSO4·3H2O(s) ↔ CuSO4·H2O(s) + 2 H2O(g) (2) (iii) NH4Cl(s) ↔ HCl(g) + NH3(g), when the equilibrium is approached by starting only with the solid.
- Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C.Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C. What is the pH of this saturated Ca(OH)2 solution?Suppose that in an industrial process, N2 at 1.00 bar is mixed with H2 at 3.00 bar, for a total pressure of 4.00 bar, and the two gases are allowed to come to equilibrium with the product ammonia in a reactor of constant volume (in the presence of a catalyst, so the reaction proceeds quickly). At the temperature of the reaction , it has been determined experimentally that K = 977 for reaction R2. What are the equilibrium partial pressures of the three gases?
- Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) A )Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc = _____/_____ = _____ Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the concentration of O₂ at equilibrium. [O₂]eq = _____MConsider the reaction. 2A(g)↽−−⇀B(g)?p=9.52×10−5 at 500 K2A(g)↽−−⇀B(g)Kp=9.52×10−5 at 500 K If a sample of A(g)A(g) at 4.20 bar4.20 bar is heated to 500 K500 K, what is the pressure of B(g)B(g) at equilibrium?Pentene (C5H10) reacts with ethanoic acid to form pentyl ethanoate, the equilibrium CH3CO2H + C5H10 ➡ CH3CO2C5H11 being established when a solution of 0.020 moles of pentene and 0.010 moles of acetic acid in 600cm3 of an inert solvent was allowed to reach equilibrium at 150C, 0.0090 moles of pentyl ethanoate was formed. Write down an expression for the equilibrium constant Kc for the above reaction.
- A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the value of KC at 800. K?Based on a Kc value of 0.170 and the data table given, what are the equilibrium conversations of XY, X, and Y, respectively?b) In a company that wants to use this gas equilibrium as a source of hydrogen gas H2, it is desired with a gas pressure of hydrogen equal to 7,850 atm. What equilibrium pressure in atm of ethanol C2H5OH is required to satisfy this requirement? c) What must the initial pressure of ethanol be to meet the requirement for 7,850 atm H2 gas at equilibrium? Supplied: Use an S E L table to organize data and set up the expression for Kc after Guldberg-Waages mass action law for the homogeneous gas equilibrium if possible, I would like handwritten answers with calculations. Thanks :)