The Equilibrium Constant
15.2.1 Select the equilibrium expression for the reaction
2CO(g) + O2(g) ⇄ 2CO2(g)
(a)
(b)
(c)
(d)
(e)
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Student Solutions Manual For Chemistry: Atoms First
- Consider the hypothetical reaction, which has an equilibrium constant (Kp) of 16.1 when the reaction occurs at 167°C. 2 W (g) + X (g) <---> 3 Y (g) If the equilibrium partial pressure of W is 0.787 atm and that of Y is 1.65 atm, what will the equilibrium partial pressure (in atm) of X be? (answer in 3 significant figures)arrow_forwardConsider the following equilibrium: 2HF(g)⇌H2(g)+F2(g) At equilibrium, the concentration of hydrogen fluoride gas, hydrogen gas, and fluorine gas are 2.04 mol/L, 2.47 mol/L, and 1.89 mol/L. What is the value of the equilibrium constant? Answer to 3 decimal places.arrow_forwardWhat is the numerical value of KcKc for the following reaction if the equilibrium mixture contains 0.32 MM CO2CO2, 0.036 MM H2H2, 0.19 MM COCO, and 0.25 MM H2OH2O? CO2(g)+H2(g)⇌CO(g)+H2O(g)CO2(g)+H2(g)⇌CO(g)+H2O(g)arrow_forward
- Consider the reaction below, for which K = 4.2 × 10–31 at 27 °C. N2 (g) + O2 (g) ⇌ 2NO (g) What is the value of K for the equilibrium below?4NO (g) ⇌ 2N2 (g) + 2O2 (g) Select one: a. 8.4 × 1031 b. 2.4 × 1030 c. 1.8 × 10–61 d. 8.4 × 10–31 e. 5.7 × 1060arrow_forwardAt 35ºC, an equilibrium mixture in a 1.0-L flask contains 0.012 mol of Cl2, 0.010 mol of NO, and 0.28 mol of NOCl. Calculate the value of equilibrium concentration (Kc) of the following reaction. 2NOCl(g) ⟷ 2NO(g) + Cl2(g) Group of answer choices A. 1.8 × 10–5 B. None of the answer choices C. 4.3 × 10–4 D. 1.5 × 10–5arrow_forwardAmmonium carbamate, NH4OCONH2, decomposes to produce ammonia and carbon dioxide. At 23.0°C the value Kp for this reaction is 6.41×10 NH4OCONH2(s)=2 NH3(g)+CO2(g) 1st attempt Part 1 A large amount of solid ammonium carbamate is placed in a rigid container at 23.00°C and allowed to come to equilibrium. What is the pressure of NH3 after equilibrium has been established? atm Part 2 What is the pressure of CO2 after equilibrium has been established?arrow_forward
- A sample of SO3 decomposes according to the following equation: 2 SO3(g) 2 SO2(g) + 1 O2(g) An equilibrium mixture in a 10-L vessel at 645 oC, contains 0.0251 g of SO3, 0.0697 g of SO2, and 0.0185 g of O2. (a) Calculate KP for this reaction at this temperature. KP = . . (b) What is the total pressure exerted by the equilibrium mixture of gases? Ptotal = Incorrect: Your answer is incorrect. atm.arrow_forwardSuppose you are given the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas B, the value of K: Select one: a. increases, because by adding A more products are made, increasing the product to reactant ratio b. does not change, as long as the temperature is constant c. depends on whether the reaction is endothermic or exothermic d. does not change, because A does not figure into the product to reactant ratio e. decreases, because A is a reactant so the product to reactant ratio decreasesarrow_forwardTopic: The State of the Equilibrium The equilibrium constant Kp for the oxidation of sulfur dioxide into sulfur trioxide is 5.6 X 104 at 350℃. If the equilibrium partial pressures of SO2 and SO3 are 0.64 atm and 0.58 atm, respectively, what is the partial pressure of O2 in the system? 2SO2(g) + O2(g) ⇌ 2SO3(g)arrow_forward
- The value of Kc = 2.20•10-10 for the equilibrium of the decomposition of phosgene is: COCl2 (g) D CO(g) + Cl2 (g) If the concentration of Cl2 at equilibrium is 4.80•10-6 M, a) What are the equilibrium concentrations of the other two substances? [CO] eq = ___________ [COCl2] eq = ___________ b) What is the initial concentration of COCl2? (Express in scientific notation) [COCl2] int = ___________arrow_forward4.4 g of CO2(g) are introduced into a 1 dm3 flask containing excess carbon at 1000oC, so that the equilibrium CO2(g) + C(s) 2 CO(g) is reached. The gas density at equilibrium corresponds to an average molecular weight of 36. Calculate the equilibrium total pressure and the value of Kp. Answer: [1408 kPa; 7.04]arrow_forwardAt a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.154. If 0.198 atm N2O4 is sealed in a flask, what partial pressure (in atm) of NO2 will exist at equilibrium? (no scientific notation)N2O4(g) ⇄ 2NO2(g)arrow_forward
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