For the reaction, N2(g) + O¿(g) = 2NO(g) K, is 0.01 at 2000 °C. After this system has established equilibrium, 0.015 moles of N2 are added. How does the addition of N2 affect the concentrations of both Oz and NO once equilibrium is established again? (A) The concentration of O2 decreases and the concentration of NO increases. (B) The concentration of O, increases and the concentration of NO decreases. (C) The concentration of O2 does not change and the concentration of NO increases. (D) The concentration of O2 decreases and the concentration of NO does not change.

For the reaction, N2(g) + O¿(g) = 2NO(g) K, is 0.01 at 2000 °C. After this system has established equilibrium, 0.015 moles of N2 are added. How does the addition of N2 affect the concentrations of both Oz and NO once equilibrium is established again? (A) The concentration of O2 decreases and the concentration of NO increases. (B) The concentration of O, increases and the concentration of NO decreases. (C) The concentration of O2 does not change and the concentration of NO increases. (D) The concentration of O2 decreases and the concentration of NO does not change.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Ammonia is produced by the following reaction: N,(g) + 3H2(g) = 2NH3(g) In an experiment, 1.00 mol of N, and 3.00 moles of H2 were allowed to react and reach equilíbrium in a sealed 5.00-L reaction vessel at 500 °C. At equilibrium, the concentration of NH, in the mixture was 0.041 M. (a) What are the equilibrium concentrations of N, and H2? (b) Calculate the equilibrium constants Ke and Kp for this reaction at 500 °C? (R = 0.0821 L.atm/Mol.K) %3D
The teeth are protected by a hard enamel layer, which is composed of a mineral called hydroxyaptite, Caş(PO4)3OH. Hydroxyaptite dissolves in saliva, as shown in the following equation: Caş(PO4);OH(s) → 5C2² + 3PO,³¯ (aq)' In adults, this process is balanced by the reverse process. (In other words, it is an equilibrium.) When you eat, food is broken down by bacteria, and acids are produced. These acids react with the hydroxide ion to form water. Explain (aq) + OH¯(aq) why this reverse process promotes tooth decay.
||| = Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 193.: CO(g) + H₂O(g) - CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 23. L reaction vessel is filled with 1.2 mol of CO₂ and 1.2 mol of H₂. 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. CO₂(g)+H₂(g) 2 CO(g) + H₂O(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 CO(g)+2H₂O(g) - 2 CO₂(g) + 2H₂(g) Exmlanation Check Q Search O There will be very little CO and H₂O. O There will be very little CO₂ and H₂. O Neither of the above is true. K = 0 K = 0 X W Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce ? S HH
Consider the decomposition reaction: X(g) + 2 Y(g) XY2(s) where X and Y are some chemical groups. At a certain temperature the equilibrium constant for this reaction is Ke= 0.108. If you start with a large amount of XY2 (s), c= what will be the concentration of Y(g) once the system reaches equilibrium? (HINT: Draw an ICE table or you will likely get this wrong!) (A) 0.108 M (B) 0.216 M (C) 0.300 M (D) 0.600 M (E) 1.08 M
Calculatıng équllibiiuml CompositiUIT iTum un Suppose a 250. mL flask is filled with 0.70 mol of O, and 1.9 mol of NO. The following reaction becomes possible: N2(3) + 0,(g) - 2NO(3) The equilibrium constant K for this reaction is 1.81 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. | M Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use
Consider the reaction: Xe(g) + 2 F2(g) ⇌ XeF4(g). A reaction mixture initially contains 1.702×103 torr Xe and 3.245×103 torr F2. If the equilibrium pressure of Xe is 258 torr, find the equilibrium constant (Kp) for the reaction.(a) 8.36×10‒4(b) 0.0395 (c) 25.3 (d) 7.52×10‒7
For the following chemical reaction, CO (g) + H2O (g) <----> CO2 (g) + H2 (g) Kc = 0.0257 If a 2.00L vessel is charged with 0.200 moles of CO, 1.13 moles of H2O, 0.199 moles of CO2, and 0.175 moles of H2, in which direction does the reaction progress to establish equilibrium?
At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.400 mol H2 and 0.400 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI]= M At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.13×10−3. At equilibrium, the concentration of AB is 2.725 M, the concentration of BC is 2.225 M, and the concentration of AC is 0.220 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq) [B]= M
Hydrogen iodide decomposes according to the reaction: 2 HI(g) = H2(g) + I2(g) At 703 K, a sealed 1.50-L container initially holds 0.00415 M H2, 0.00276 M I2, and 0.0163 M HI When equilibrium is reached, the equilibrium concentration of H2(g) is 0.00467 M. What is the equilibrium concentration of HI(g)? None of these 0.00328 M 0.00052 M 0.0158 M 0.0173 M 0.0153 M
(a) At 2000°C, the equilibrium constant for the reaction: N2(g) + O2(g) > 2 NO(g) is 4.1 x 10-4 If the initial concentration are [N2] = 0.2 M and [O2] = 0.1 M, how much of each of the components will be present at equilibrium?
The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?
At a certain temperature, the equilibrium constant K for the following reaction is 6.0 x 10: co(e) + H,0(g) -co,() + H,(g) Use this information to complete the following table. Suppose a 31. L reaction vessel is filled with 1.1 mol of co, and 1.1 mol of H2. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little CO and H,0. O There will be very little Co, and H,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] Co,(0)+H,(0) CO()+H,O(9) 1. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 3 CO0g)+3H,0(9) 3 CO,(0)+3H,(9) 1.