The equilibrium constant for the following reaction is 6.50×10*³ at 298K. 2NOBr(g)=2NO(g) + Br2(g) If an equilibrium mixture of the three gases at 298K contains 2.19×10-2 M NOBr(g) and 3.60×10² M NO, what is the equilibrium concentration of Br2? M Submit Answer Retry Entire Group 9 more group attempts remaining

The equilibrium constant for the following reaction is 6.50×10*³ at 298K. 2NOBr(g)=2NO(g) + Br2(g) If an equilibrium mixture of the three gases at 298K contains 2.19×10-2 M NOBr(g) and 3.60×10² M NO, what is the equilibrium concentration of Br2? M Submit Answer Retry Entire Group 9 more group attempts remaining

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

Dear expert don't use Ai plz 2 downvotes
7 $ R Q Consider the following system at equilibrium where AH° = 16.1 kJ/mol, and Kc = 6.50x10-3, at 298 K. 2 NOBr (g) 2 NO (g) + Br₂ (g) When 0.19 moles of NOBr (g) are added to the equilibrium system at constant temperature: The value of Kel The value of Qcl % 5 The reaction must Orun in the forward direction to restablish equilibrium. Orun the reverse direction to restablish equilibrium. O remain the same. It is already at equilibrium. The concentration of NO will ✔ Use the References to access important values if needed for this question. T G Submit Answer B e F5 A 6 Y H FO N Retry Entire Group & 7 K Kc. F7 U * 8 M DII FB 1 References 9 more group attempts remaining K ( 9 DD O O F10 P F11 Previous Next> { F12 delete
At 1100 K, Kp = 0.32 for the reaction 2SO₂(g) + O₂(g) ⇒ 2SO3 (9) What is the value of K at this temperature? K= Submit Answer Try Another Version 1 item attempt remaining
[References] The equilibrium constant (K.) for the reaction PC13 (g) + Cl2 (g) =PCl; (g) equals 49 at 230°C. If 0.107 mol each of phosphorus trichloride and chlorine are added to a 8.60 L reaction vessel, what is the equilibrium composition of the mixture at 230°C? mol PC13 mol Cl2 mol PCI5 Submit Answer
View Policies Current Attempt in Progress Examine the following reaction. 3 CO 2(8)+2 Fe(s) Fe 203(s) +3 CO(g) What is the equilibrium expression for the reaction? O K = [Fe,O3][CO18 / ([Fe]? [CO,1) O K = [CO2)/[CO] OK = [CO2]8 /[cOJ O K = (Fe]/[Fe2O3] O K = [CO]/[CO2) O K= [Fe,O3][CO]/ ([Fe] [CO,) O K = [Fe2O3]/[Fe] O K = [Fe] [CO2)/ ([Fe,O3] [CO]) O K = [CO] /[CO2] O K = (Fe] [CO21³/ ((Fe,O3] [CO]³) %3D %3D !! Save for Later
A closed system at 150 °C initially contained 10 g of NH4Cl(s) before reaching equilibrium. The equilibrium constant is Kp = 1.7 x 10-7 for the reaction. NH4Cl(s) ⇒ NH3(g) + HCl(g) What is the partial pressure of HCI at equilibrium? (A) 0.85 x 10-2 Pa 【(B) 1.7 × 10-² Pa (C) 41 Pa (D) 4.1 x 104 Pa (E) 21 Pa
10) The reaction A2 + B2 = 2 AB has an equilibrium constant Kc = 9.0. The following pictures represent %3D 10) reaction mixtures that contain A2 molecules (shaded) and B2 molecules (unshaded), and AB molecules. Which reaction mixture is at equilibrium? 8. 00 (1) (2) (3) (4) A) reaction mixture (1) C) reaction mixture (3) B) reaction mixture (2) D) reaction mixture (4)
K=4.9x10-3 for the reaction CO2(g)+H2(g)⇄ CO(g)+H2O(g). If [CO2]=0.00025 M, [H2]=0.0010 M, & [CO]=0.000015 M, what is the concentration at equilibrium of H2O? Answer 8.2x10-5M I got 1.84x10^-14? Can someone explain this to me please.
D.8.
pls help me thank u
As an environmental chemist you are studying formation of carbon monoxide, The following equilibrium constants were determine at 35°C:. (1) 2 C (s) + O2 (2) + 2 CO (2) Ke = 4.80 e-10 (2) 2 CO2 (e + 2 CO (g) + O2 (e) K = 1.10 e-5 i) Find Ke for CO2 1g) → C (s) + O2 (6) at 35°C ?
Show work..don't give Handwritten answer..don't use Ai for answering this