20. Given the equilibrium reaction PCI5 (g) → PC13 (g) + Cl2 (g) Calculate the number of moles of C12 produced at equilibrium when 1.00 mol of PCI5 is heated at 246.9 deg celsius in a vessel having a capacity of 10.0L. At 246.9, K = 0.053 for this dissociation.
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- The equilibrium constant (K1) for the reaction CO2 (g) 2 CO(g)+1/2 O2(g) is 6.66 x 10-12 at 1000 K. Calculate K2 for the reaction CO(g) +1/2 0,(g) 2 CO2 (g) K2 = %3DExactly 1.0 mol N,04 is placed in an empty 1.O-L container and allowed to reach equilibrium described by the equation N204(s) = 2NO,(g). If at equilibrium the N,04 is 28.0% dissociated, what is the value of the equilibrium constant, K. for the reaction under these conditions? 0.44 O 2.3 0.31 0.78 0.11A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous NO was present. Assume that the reaction SO-(9) + NO2 (g) = SO; (g) + NO(9) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K =
- The equilibrium constant K. for the equation CS2 (9) + 4H, (9) # CH4 (9) + 2H, S(g9) at 900°C is 27.8. What is the value of K. for the following equation? | CH, (9)+1H2 S(9) = Cs, (9)+2Hz (9) Ke6.) 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)Calculate the value of the equilibrium constant, Ke, for the reaction Q(g) + X(g) = 2 M(g) + N(g) given that M(g) Z(g) 6 R(g) = 2 N(g) +4Z(g) 3 X(g) +3Q(g) 9 R(g) Kel 3.88 Kez = 0.445 %3D Ke3 = 13.5 %3D
- Given C₂H6O(g) + 302(g) = 2CO2(g) + 3H₂O(g) 2C₂H4G(g) +502(g) = 4CO2(g) + 4H₂O(g) calculate the equilibrium constant for 2C₂H6O(g) + O2(g) = 2C₂H4O(g) + 2H₂O(g) K₂= 7.2 Kp= 7.1 × 101 Report your answer with two significant figures. Do NOT include units in your answer.Consider the reaction: N2(g) + 3H2(g) 2NH3(g) where Kc = 0.500 at 400 °C. If 50.0 L reaction vessel contains 1.000 mole N₂; 3.000 mole H₂ and 0.050 mole NH3, which of the following is TRUE? The reaction based on the following parameters is in equilibrium. More ammonia will be produced as the reaction approaches equilibrium. Data provided is not enough to warrant a conclusion regarding equilibrium. More ammonia will dissociate as the reaction approaches equilibrium.Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400° C established the concentration of N, to be 1.2 M and the concentration of H, to be 0.24 M. N,(g) +3H,(g) =2NH;(g)K¸=0.50 at 400° C. What is the equilibrium molar concentration of NH, 13? A 0.091 B 0.0091 0.0083 0.24
- 1.25 moles of NOClwere placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, Kc, for the reaction 2NOCl(g) -> 2NO(g) + Cl2(g).Given the following reactions and the equilibrium constants CO (g) + H,0 (g) Co, (g) + H2 (g) K1 = 1.0 X 105 co (g) + 2 H2 (g) CH;OH (g) K2 = 1.4 X 107 Predict the equilibrium constant for Co, (g) + 3 H, (g) CH;OH (g) + H,0 (g) K = ? 4 O 13900000 O 140 O 0.007146) 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 = ?