A 4.00 L flask at 25 °C is filled with 0.266 moles of X2 and 0.344 moles of Y2 and allowed to react according to the following reaction: 3X2 (g) +Y 2 (g) –→ 2Y X3 (g) When the reaction reaches equilibrium it has 0.0465 moles of YX3, what is the equilibrium constant Kc at 25 °C? O 1.34 O 14.3 O 2.95 O 0.0701 O 0.00581

When 3.00 mol of A and 1.00 mol of B are mixed in a 1.00 L vessel, the following reaction takes place: A(g) + B(g) →2 C(g). The equilibrium mixture contains 0.50 mol of C. What is the value of the equilibrium constant for the reaction? 0.24 8.3 O 0.20 0.12

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BA

Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 1.22×10-2 moles of COCl2(g), 0.591 moles of CO, and 0.561 moles of Cl2 are at equilibrium in a 15.3 L container at 789 K, the value of the equilibrium constant, Kc, is