A student ran the following reaction in the laboratory at 325 K: 2NO(g) + Br2(g) 2NOBr(g) When she introduced 0.102 moles of NO(g) and 9.44×102 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 7.16х10? м. Calculate the equilibrium constant, Ke, she obtained for this reaction. K =

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 =

Please answer with the correct number of significant digits. At a certain temperature, the equilibrium constant K for the following reaction is 9.7 x 10¹¹: NO₂(g) + CO(g) NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 42. L reaction vessel is filled with 1.2 mol of NO₂ and 1.2 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(9) 1 NO₂(9)+CO (9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 NO₂(9)+2CO(g) 1 2 NO(g) +2C0₂(9) There will be very little NO₂ and CO. There will be very little NO and CO₂. Neither of the above is true. K-O K-0 X

A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр

At a certain temperature, the equilibrium constant K for the following reaction is 6.09 × 10 °: N,(3) + O,(g) =2 NO(g) Use this information to complete the following table. Suppose a 28. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N2 and O2. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2 NO(g) N3(9)+O2(9) 1L What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] 2N2(9)+20,(9) 4 NO(g)

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 377 K: CH₂(g) + CCL (9) ⇒ 2CH₂Cl2 (9) When she introduced 0.0391 moles of CH4 (g) and 0.0708 moles of 14 CCl4 (g) into a 1.00 liter container, she found the equilibrium concentration of CCl4 (g) to be 0.0623 M. Calculate the equilibrium constant, Ko, she obtained for this reaction. Kc =

Using the general properties of equilibrium constants 0/5 At a certain temperature, the equilibrium constant K for the following reaction is 7.4 × 10 ': N,(e) + 0,(g) -2NO(g) Use this information to complete the following table. Suppose a 35. L reaction vessel is filled with 1.7 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little N, and 0,. O There will be very little NO. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =] 2 NO(g) N2(0)+O2(a) 1, What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 2N,(0)+20,(0) 4 NO(g) 1,

A chemical engineer is studying the following reaction: 2 NO(g)+2H,(9) - N2(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel ΝΟ 6.78 atm O f increase Ot decrease O (no change) H, 2.93 atm ↑ increase OI decrease O (no change) A N2 5.23 atm f increase I decrease (no change) H, O 7.24 atm t increase I decrease (no change) NO 5.29 atm f increase I decrease (no change) H, 1.44 atm f increase OI decrease (no change) В N2 5.98 atm increase I decrease (no change) H, O 8.73 atm f increase O I decrease O (no change)…

A student ran the following reaction in the laboratory at 675 K: H2(g) + I2(g) 2HI(g) When she introduced 0.226 moles of H2(g) and 0.248 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.11×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =