Dinitrogen tetraoxide, a colorless gas, exists in equilibrium with nitrogen dioxide, a reddish brown gas. One way to represent this equilibrium is: 2NO2(g)N,04(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1/2 K1 1) N,04(9) (5)-ON = K2 1/2 2) NO2(g) N204(g) K3 3) N204(g) = 2NO2(g) II

Dinitrogen tetraoxide, a colorless gas, exists in equilibrium with nitrogen dioxide, a reddish brown gas. One way to represent this equilibrium is: 2NO2(g)N,04(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1/2 K1 1) N,04(9) (5)-ON = K2 1/2 2) NO2(g) N204(g) K3 3) N204(g) = 2NO2(g) II

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

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 2.0 mol of NO, and 1.3 mol of NO. The following reaction becomes possible: NO, (g) + NO(g) → 2NO, (g) The equilibrium constant K for this reaction is 6.91 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use |P 21
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) CO(g) + Cl2(g) ⟷ COCl2(g)If the equilibrium constant for this reaction is Kc = 248, predict what will happen when [CO] = [Cl2] = [COCl2] = 0.0200 M. Group of answers The reaction will proceed in the forward direction to reach equilibrium. The reaction is at equilibrium already before every substance is at the same concentration. Because K > 1, the reaction will proceed in the forward direction to reach equilibrium. The reaction will proceed in the reverse direction to reach equilibrium. The temperature needs to be specified before a prediction can be made.
Consider the following reaction: CO(g) + 2 H₂ (g) CH₂OH(g) A reaction mixture in a 5.23-L, flask at a certain temperature initially contains 27.4 g CO and 2.34 g H₂. At equilibrium, the flask contains 8.65 g CH₂OH You may want to reference (Page) Section 15.8 while completing this problem Y Part A Calculate the equilibrium constant (K) for the reaction at this temperature. 15] ΑΣΦ/ Ke= Submit Request Answer
Dinitrogen tetraoxide, a colorless gas, exists in equilibrium with nitrogen dioxide, a reddish brown gas. One way to represent this equilibrium is: N,04(g)2NO,(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) NO2(g) =1/2 N204(g) K = 2) 2NO2(g) = N204(g) K2 = 3) 1/2 N204(g) : NO2(g) K3 = Drag and drop your selection from the following list to complete the answer: (1/K)!2 K12 1/K
For the reaction : 4Al + 3O2 ⇆ 2Al2O3 the equilibrium concentrations are [Al2O3] = 67.3 mol/L, [Al] = 0.64 mol/L, and [O2] = 0.64 mol/L. Write the equilibrium expression and calculate the equilibrium constant, K. Are products or reactants favored? If the reaction is at equilibrium, and we increase the concentration of Al2O3, in which direction will the reaction move (left or right)? If the reaction is endothermic and we increase the temperature, which direction will the equilibrium shift? Left or right? Why?
Phosgene is a chemical warfare agent first used on soldiers in World War I. It is synthesized according to the following gas-phase equilibrium reaction: CO(g) + Cl, (g) = COCI,(g) Write the equilibrium expression K, for this reaction below. K. = If K. = 0.281 for this reaction, would the product or the reactant be favored at equilibrium? The reactants would be favored. Neither the product nor the reactants would be favored. The product would be favored.
@quinnipiac.edu doesn't allow editing on a Mac. To learn more, contact your admin about your Office plan. 4. What is the correct equilibrium constant (K.) expression for the following reaction? Fe2O3(s) + 3H2(g) 2 2Fe(s) + 3H20(g)
For the chemical equilibrium N₂ + 3H22NH3 what is the expression for the equilibrium constant? K=
4.
Consider the reaction: 2 CO(g) + O2(g)=2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.
4) When the pressure of the following mixture of gases is decreased, what will be the effect on the equilibrium position? HCI (9) + O2 (g) → H2O (g) + Cl2 (9)
Consider the following reaction: A (g) + B (g) 2 C (g) + D (g) A reaction mixture initially contains 2.5 M A and 2.0 M B. If the equilibrium concentration of C is 1.8 M, what is the value of the equilibrium constant (Kc) for the reaction?