ieht 15.8 - Enhanced - with Feedback Part A MISSED THIS? Watch KCV 15.8, IWE 15.12; Read Section 15.8. You can click on the Review link to access the section in your eText. What is the concentration of B when the reaction reaches equilibrium? Consider the reaction of A to form B: 2 A (g) =B (g) K. = 2.4 × 10 5 (at 298 K) O 3.1 x 10-5 M A reaction mixture at 298 K initially contains [A] = 0.80 O 3.8 x 10-5M M.

ieht 15.8 - Enhanced - with Feedback Part A MISSED THIS? Watch KCV 15.8, IWE 15.12; Read Section 15.8. You can click on the Review link to access the section in your eText. What is the concentration of B when the reaction reaches equilibrium? Consider the reaction of A to form B: 2 A (g) =B (g) K. = 2.4 × 10 5 (at 298 K) O 3.1 x 10-5 M A reaction mixture at 298 K initially contains [A] = 0.80 O 3.8 x 10-5M M.

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 84AE: At 25C. Kp 1 1031 for the reaction a. Calculate the concentration of NO, in molecules/cm3, that can...

See similar textbooks

Similar questions

At 25C. Kp 1 1031 for the reaction a. Calculate the concentration of NO, in molecules/cm3, that can exist in equilibrium in air at 25C. In air, PN2=0.8 atm and PO2=0.2atm. b. Typical concentrations of NO in relatively pristine environments range from 108 to 1010 molecules/cm3 Why is there a discrepancy between these values and your answer to part a?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
The equilibrium constant for the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g)N2(g)+3H2(g)↽−−⇀2NH3(g) is ?p=0.0703Kp=0.0703 at 237 °C237 °C . Calculate the value of the ?cKc for the reaction at 237 °C237 °C .
Nitrogen dioxide exists in equilibrium with dinitrogen tetroxide: N2O4 (g) = 2 NO2 (g) At 25oC and a pressure of 0.597 bar the density of the gas is 1.477 g dm-3 . Calculate the degree of dissociation under these conditions, and the equilibrium constant KP. Answer: [0.5; 0.795 bar]
An equilibrium mixture from the following reaction was found to contain 1.20 mol dm-3 of A, 1.00 mol dm-3 of B, and 0.80 mol dm-3 of C. A (g) ⇌ B (g) + C (g) a. What is the value of Kc for this reaction? b. If the volume of the reaction vessel were suddenly doubled while the temperature remained constant, determine whether the system be at equilibrium. If not, what must occur to establish equilibrium? c. If the initial volume of the reaction vessel were halved, while the temperature remains constant, determine whether the system be at equilibrium. If not, what must occur to establish equilibrium?
What is the equilibrium constant for a reaction at temperature 59.3 °C if the equilibrium constant at 25.7 °C is 30.3? Express your answer to at least two significant figures. For this reaction, ΔrH° = -4.2 kJ mol-1.
3 (i) In the Haber process for the production of ammonia, the following reaction occurs: N2 (g) + 3H2 (g) 2NH3 (g) DH is negative If the equilibrium concentrations for all the reactants and products at 6000C are: [N2] = 0.40 mol/dm3, [H2] = 1.20 mol/dm3 and [NH3] = 0.20 mol/ dm3 Construct an expression for Kc and calculate the numerical value of the equilibrium constant, Kc (ii) At 5000C Kc = 0.062 mol-2dm6. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 5000C or 6000C and briefly explain your choice.
the equilibrium constant for the reaction at 385 K is 2.78·10-4. Calculate the equilibrium constant for that reaction at a temperature of 345 K, when the reaction's ΔH° = 41 kJmol-1. ΔH° is assumed to be independent of temperature
At 500 K, the following concentrations were measured for the following reaction: 2NH3 (g) ⇌ N2 (g) + 3H2 (g) [N2] = 3.0 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M Calculate Kc.
Calculate delta G for the reaction, 2A (g) + B2(g) —- 2AB(g) given that at 120 C the equilibrium constant of the reaction is 3.12 x 10^5 -41.43 j/mol -41.43 kj/mol None of the above -35.76 kj/mol -414.30 j/mol
(a) If Qc > Kc, how must the reaction proceed to reachequilibrium? (b) At the start of a certain reaction, onlyreactants are present; no products have been formed.What is the value of Qc at this point in the reaction?
Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2.N2O4 (g) ⇌ 2 NO2 (g) (a) The equilibrium constant Kc at 25°C is 0,125. What percentage of dinitrogen tetroxideis dissociated when 0,0300 mol N2O4 is placed in a 1,00 dm3 flask and left to reachequilibrium?