The image presents two chemical reactions with their respective equilibrium constants:1. \( \text{A} + 2\text{B} \rightleftharpoons 2\text{C} \) with equilibrium constant \( K_1 = 2.81 \).2. \( 2\text{C} \rightleftharpoons \text{D} \) with equilibrium constant \( K_2 = 0.248 \).The task is to calculate the value of the equilibrium constant for the reverse reaction:\[ \text{D} \rightleftharpoons \text{A} + 2\text{B} \]The result of the calculation should be entered in the provided space labeled:\[ K = \] **Explanation for Calculation:**To find the equilibrium constant for the reverse reaction \( \text{D} \rightleftharpoons \text{A} + 2\text{B} \), the following relationship is used:\[ K_{\text{reverse}} = \frac{1}{K_{\text{forward}}} \]Thus, we first need to determine \( K_{\text{forward}} \) for the reaction \( \text{D} \rightleftharpoons \text{A} + 2\text{B} \), which can be found by combining the given reactions.1. Reverse the second reaction to get \( \text{C} \rightleftharpoons \frac{1}{2}\text{D} \), where the equilibrium constant becomes \( \frac{1}{K_2} = \frac{1}{0.248} \).2. The overall reaction is obtained by combining these adjusted reactions to yield \( \text{D} \rightleftharpoons \text{A} + 2\text{B} \).3. The equilibrium constant for the overall reaction is calculated by multiplying the modified constants \( K_1 \) and \( \frac{1}{K_2} \).Finally, take the reciprocal of this equilibrium constant to find \( K \) for the reverse reaction.

Consider the given equilibrium reaction is as follows; A + 2B ⇌ 2C K1=2.81…

Answered: Two reactions and their equilibrium…

Two reactions and their equilibrium constants are given. A+2B 2C K = 2.81 2C D K2 5 = 0.248 Calculate the value of the equilibrium constant for the reaction D=A+2B. K =

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

10. What is the expression for the equilibrium constant (K) for the reaction 2 C₂H(g) +7 O2(g) → 4 CO2(g) + 6 H₂O(g)? Tool Box: 1 cal 4.184 J 1Kcal 4.184 KJ 1000 cal 1 Kcal 1000 J = 1 KJ
Enter your answer in the provided box. Pure phosgene gas (COCI₂), 0.0220 mol, was placed in a 1.50-L container. It was heated to 720.0 K, and at equilibrium, the pressure of CO was found to be 0.503 atm. Calculate the equilibrium constant Kp for the reaction. Kp CO(g) + Cl₂(g) = COCI₂(g)
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,O4(2) (5)-ON = K2 1/2 2) NO2(g) N204(g) K3 3) N204(g) = 2NO2(g) Drag and drop your selection from the following list to complete the answer: (1К)12 K12 1/K
51.0 g of Y(g) (molar mass = 28.32 g/mol) is placed in a 0.617 L flask for the following reaction to take place. Calculate the concentration (molarity) of Z equilibrium. The equilibrium constant for the reaction is K = 4.63 x 10-4 at 25°C. Report your answer to the thousandths place. Y(g) = 2 Z(g)
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
For the chemical equilibrium N₂ + 3H22NH3 what is the expression for the equilibrium constant? K=
Kc=?
Calculate the equilibrium partial pressure of CO2.
The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.
Consider the following equilibria at a given temperature: ½Nalg) + J½O>(g) = NO(g) K= 6.45 x 10°, NO (g) + 1½Brz(g) = NOB((g) K= 1.40 Determine the value of the equilibrium constant for the following reaction at the same temperature: %N(g) + ½Ozlg) + ½Br2(g) = NOBr(g) OA 583 x 107 O B.3.36 x 10-18 OC4.17x 107 OD.6.45 x 10 OE 9.03 x 10
Find the attached image to answer the question.