A student ran the following reaction in the laboratory at 652 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.25×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 7.26×10-3 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

Consider the following reaction and its equilibrium constant: 12 (g) + Br2 (g) ÷ 2 IBr (g) Kc = 1.1 × 102 A reaction mixture contains 0.41 M I2, 0.27 M Br2 and 2.2 M IBr. Which of the following statements is TRUE concerning this system? O The equilibrium constant needs to increase. The reaction needs to shift in the direction of the reactants to reach equilibrium. O The system is at equilibrium. O The reaction needs to shift in the direction of the products to reach equilibrium.

A student ran the following reaction in the laboratory at 538 K:COCl2(g) CO(g) + Cl2(g)When she introduced 1.24 moles of COCl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.76×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.Kc =

A student ran the following reaction in the laboratory at 1083 K: 2503(g) 2sO2(g) + 02(g) When she introduced 7.36x10-2 moles of SO3(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.23x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc II

Calculating an equilibrium constant from a partial equilibrium composition Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 25.0 L tank with 2.4 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 0.36 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = x10 × Ś olo 18 Ar 8.

The equilibrium constant (K) of the reaction below is K = 2.5 x 10-3, with initial concentrations as follows: [H₂] = 1.0 x 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10 4 M. N2(g) + 3 H₂(g) 2 NH3(g) If the concentration of the reactant H₂ was increased from 1.0 x 10-2 M to 2.5 x 10- 1M, then the reaction quotient (Q) ip. [Report your answer in scientific notation] towards the The equilibrium position would shift [left/right/or remain unchanged].

A student ran the following reaction in the laboratory at 290 K:2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 8.37×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 6.14×10-3M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

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

A student ran the following reaction in the laboratory at 700 K: N2 (g) + 3H₂(g) — 2NH3 (9) When she introduced 0.0350 moles of N₂(g) and 0.0529 moles of H₂(g) into a 1.00 liter container, she found the equilibrium concentration of H₂(g) to be 0.0512 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Ke = |

A student ran the following reaction in the laboratory at 286 K:2CH2Cl2(g) CH4(g) + CCl4(g)When she introduced 6.64×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.09×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.Kc =