Determine la constante de equilibrio de la reacción AB2(g) + B(g) →→ AB3(g) usando las reacciones A(g) + 2 B(g) → AB2(g) Kc = 59 A(g) + 3 B(g) → AB3(g) Kc = 478. O a) 3.5 x 10-5 Ob) 2.8 x 104 O c) 8.1 O d) 0.12 O e) 89
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![Determine la constante de equilibrio de la reacción
AB2(g) + B(g) →→ AB3(g)
usando las reacciones
A(g) + 2 B(g) → AB2(g) Kc = 59
A(g) + 3 B(g) → AB3(g) Kc = 478.
O
a) 3.5 x 10-5
Ob) 2.8 x 104
Oc) 8.1
O d) 0.12
O e) 89](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded8214d-421f-4218-8180-ec6ab62a4773%2F8756eb79-1443-42e4-a03c-c72a9031e520%2Fuxlg0zd_processed.jpeg&w=3840&q=75)
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- Use the data shown here to find the equilibrium constant (Kc) for the reaction, A(g) → 2 B(g) +C(g) A(g) +2 X(g) +C(g) B(g) → X(g) O 984 O 26.8 O 6.10 x 10-4 O 10 O 244x103 Kc = 1.55 Kc =25.2Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 5.00 L flask at 1200 K. The flask is found to contain 2.81 g of CH, 1.25 g of CO, 15.1 g of cO, and 25.3 g of H, What is the value of Kc for this reaction? CH.(g) + CO,(9) = 2 CO(g) + 2 H,(g)6.) Given the following information: 2 A(g) + B(g) = A¿B(g) 2 A(g) + C2(g) = 2 AC(g) K1 = 5.0 x 104 K2 = 3.2 x 103 What is the net equilibrium constant (Knet) for the reaction? 2AC(g) + 4A(g)+ 3B(g)→ 3 A¿B(g) + C2(g)
- 9)Diethyl ether is a volatile, highly flammable organic liquid that is used mainly as a solvent. The vapor pressure of diethyl ether is 401 mmHg at 18 degrees C. Calculate its vapor pressure at 52 degrees C. 10) From the Haber synthesis, at the start of a reaction there are 0.249 mol N2, 3.21 X 10-2 mol H2 and 6.42 X 10-4 mol NH3 in a 3.50 L reaction vessel at 375oC. If the equilibrium constant Kc for the reaction is 1.2 at this temperature, decide whether the system 2 #3 $ 4 % 5 MacBook Pro 6 & 7 *00 I 86.) Given the following information: 2 A(g) + B(g) = A¿B(g) 2 A(g) + C2(g) = 2 AC(g) K1 = 5.0 x 104 K2 = 3.2 x 103 %3D What is the net equilibrium constant (Knet) for the reaction? 2AC(g) + 4A(g)+ 3B(g) = 3 A2B(g) + CAg)From the following equilibrium reactions: 2SO2(g) + O2(g) → 2SO3(g) K1 2C0(g) + O2(g) → 2C02(g) K2 Determine the equilibrium constant, K, for 2SO2(g) + 2CO2(g) 2SO3(g) + 2CO(g) O K=Kq/K2 O K=K1 + 1/K2 O K=K2/K1 O K=K¼×K2
- Calculate the value of the equilibrium constant (Keg) for the following reaction: 2 CO (g) + 6 H2 (g) → 2 CH4 (g) + 2 H2O (g) The following two equilibrium reactions should be helpful in determining this value: CO (g) + 2 H2S (g) <→ CS2 (g) + H2O (g) + H2 (g) ½ CH4 (g) + H2S (g) <→ ½ CS2 (g) + 2 H2 (g) Reaction 1: K1 = 1.3 x 105 Reaction 2: K2 = 180 (A) 2.3 x 107 (B) 1.9 x108 (C) (D) 16.1 722 (E) 1.5 x 10-86) A mixture of 9.00 moles of A, 10.00 moles of B, and 28 moles of C is placed in a one liter container at room temperature. The reaction is allowed to reach equilibrium at which point the number of moles of B is 18.00. Calculate the equilibrium constant, Kc, for this reaction: A (g) + 2 B (g) « 3 C (g)Kc = ?Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g) 6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?
- The equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)A sample of phosgene is sealed in a 250.0-cm³ glass bulb to which a pressure gauge is attached. The bulb is heated to 600 °C, and the gauge shows that the pressure in the bulb rises to 0.973 atm. At this temperature, the COCI₂(g) is partially dissociated into CO(g) and Cl₂(9) according to the equation CoCl₂(g) CO(g) + Cl₂(9) At 600 °C, Kp = 5.00 for this reaction. Assume that the contents of the bulb are at equilibrium and calculate the partial pressure the three different chemical species in the vessel. Pcocl₂ = Pco= Pc₂" atm atm atmConsider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled with 2.00 mol SO2 and 2.00 mol NO2 and allowed to react at a high temperature. At equilibrium, there were 1.30 mol of NO in the vessel. Determine the concentrations of all reactants and products at equilibrium and then calculate the value of Kc for this reaction. SO2(9) + NO2(g) SO3(g) + NO(g) 1 NEXT Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. SO2(g) NO2(g) SO3(g) NO(g) + Initial (M) 2.00 2.00 Change (M) -1.30 -1.30 1.30 1.30 Equilibrium (M) 0.70 0.70 1.30 1.30 RESET +x -X 1.00 2.00 1.30 -1.00 -1.30 2.30 2.70 0.70 1.35 2.00 - x 2.00 +x
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