Consider the following equilibrium: N₂(g) + 3H₂(g) 2NH, (e) AG--34. K Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 8.20 atms of ammonia (NH,) at 814. "C. Answer the following questions about this system: a Under these conditions, will the pressure of H, tend to rise or fall? Is it possible to reverse this tendency by adding N₂ In other words, if you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding Ny? Similarly, if you said the pressure of H₂ will tend to fall, can that be changed to a tendency to rise by adding N₂ If you said the tendency can be reversed in the second question, calculate the minimum pressure of Ny needed to reverse it. Round your answer to 2 significant digits. Orie fall O yes no D.P X

O O Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 0.0074: N,(g) + 0,(g) = 2NO(g) Use this information to complete the following table. Suppose a 22. L reaction vessel is filled with 0.89 mol of N, and 0.89 mol of O2. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. 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(9)+O2(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =] 2N2(9)+202(g) 4 NO(g) 1. Explanation Check 02021 McGraw-Hill Education All Rights Reserved Terms of U

KINETICS AND EQUILIBRIUM Using an equilibrium constant to predict the direction of... A chemical engineer is studying the following reaction: 4 HC1(g) + O₂(g) → 2 H₂O(g) + 2Cl₂(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.31. The engineer charges ("fills") four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel A B с compound HC1 0₂ H₂O Cl₂ HCI 0₂ H₂O Cl₂ HCI 0₂ H₂O C1₂ pressure 5.09 atm 5.63 atm 3.31 atm 4.48 atm 3.91 atm 5.34 atm 3.90 atm 5.07 atm 2.74 atm 5.05 atm 4.48 atm 5.65 atm expected change in pressure O ↑ increase ↑ increase O ↑ increase O ↑ increase O ↑ increase ↑ increase ↑ increase O ↑ increase ↑ increase O ↑ increase ↑ increase ↑…

Nitrogen monoxide and water react to form ammonla and oxygen, Ilke this: 4 NO(g) + 6H,O() 4 NH,(g) + 50,(g) Also, a chemist finds that at a certain temperature the equilibrlum mixture of nitrogen monoxide, water, ammonia, and oxygen has the followng composition: compound pressure at equilibrium NO 12.7 atm H,0 94.3 atm NH3 58.1 atm 0, 93.8 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. d. K = x10 Check Explanation ©2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Ac M9 hp & esc % * 00 96 %24

At a certain temperature, 0.88 mol N, and 2.654 mol H, are placed in a container. N2 (g) + 3H, (g) = 2NH; (g) At equilibrium, there is 0.82 mol NH, present. Determine the number of moles of N, and H, that are present when the reaction is at equilibrium. moles of N, at equilibrium: mol moles of H, at equilibrium: mol | privacy policy terms of use | help about us careers contact us O Ei A Gateway

Suppose a 500. mL flask is filled with 0.40 mol of N, and 0.10 mol of 0,. The following reaction becomes possible: N, (g) + 0,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.29 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places. OM

Nitrogen 2NF3(g)->N2(g) + 3F2(g) When 3.15 mol of NF3 is placed in a 3.00-L container and allowed to come to equilibrium at 900 K, the mixture is found to contain 0.0563 mol of N2. What is the value of K, at this temperature? (R = 0.0821 L'atm-mol¹ K¹). (Hint: Solve for Kc first, then calculate Kp) 4.43 x 10-7 1.8 x 102 1.11 x 10-5 191 x 103 1.07 x 10-5