At a particular temperature, K = 3.1 for the reaction SO2 (9) + NO2(9) SO3(9) + NO(9) If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases. [SO2] = м [NO2] = M [SO3] = M %3! [NO] = %3! Submit Answer Try Another Version 3 item attempts remaining

At a particular temperature, K = 3.1 for the reaction SO2 (9) + NO2(9) SO3(9) + NO(9) If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases. [SO2] = м [NO2] = M [SO3] = M %3! [NO] = %3! Submit Answer Try Another Version 3 item attempts remaining

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.95QE: Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration...

See similar textbooks

Similar questions

At 100 ∘C∘C, Kc=0.078Kc=0.078 for the reactionSO2Cl2(g)←→SO2(g)+Cl2(g)SO2Cl2(g)←→SO2(g)+Cl2(g)In an equilibrium mixture of three gases, the concentrations of SO2Cl2SO2Cl2 22 and SO2SO2 are 0.150 MM and 0.145 MM respectively. What is the partial pressure of Cl2Cl2 in the equilibrium mixture? Express your answer using two significant figures.
The equilibrium constant, Kc is 0.0183 for the reaction at a certain temperature: 2 HI(g) ⇄ H2(g) + I2(g) If 3.00 moles of HI are placed in a 5.00 L vessel and allowed to reach equilibrium, what is the equilibrium concentration (in mol/L) of H2 gas? Hint: use the perfect square method and construct an ICE table. Record your answer as a standard number to 3 significant figures. For example, if the answer is 2.75 x 10-3 mol/L then you should enter 0.00275 as the answer.
Kc = 0.040 for the system below at 450 oC. If a reaction is initiated with 0.40 mole of Cl2 and 0.40 mole of PCl3 in a 2.0 liter container, what is the equilibrium concentration of Cl2 in the same system? PCl5(g) ⇌ PCl3(g) + Cl2(g) This question was answered but I coudn't read the solution. It was all jumbled up. I've included a picture of the answered question below for review. Can you please make it more coherent?
Suppose a mixture was prepared containing 0.0100 mol H2, 0.0150 mol F2, and 0.0180 mol HF in a 1.25 L reaction vessel. What will the concentrations of all the gases be when equilibrium is reached? The reaction is 2HF(g) H2(g) + F2(g) for which the equilibrium constant Kc = 1.2 × 10-13. If any value is actually very small, put zero in your answer. Concentration of HF at equilibrium? ____M Concentration of H2 at equilibrium? ___M Concentration of F2 at equilibrium? ___M
For the reaction 3H2(g)+N2(g)⇌2NH3(g) at 225 ∘C the equilibrium contant is 1.7×10 ^2. If the equilibrium mixture contains 0.19 M H2 and 0.015 M N2, what is the molar concentration of NH3? Express your answer to two significant figures and include the appropriate units.
You're provided with a bottle labled [CoCl2.6H2O] = 0.062 M in 4.70 M HCl. You heat a small volume of the solution in a hot water bath to 50 ∘C. If you determine that [CoCl42-] = 0.034 M at 50 ∘C at equilibrium, what must be the equilibrium concentration of [Cl-] at 50 ∘C? Express your response in units of M to three digits after the decimal. DO NOT do 4.70-(2 x 0.034) because it is wrong
At 2000 K, the equilibrium constant, Kc for the decomposition of hydrochloric acid is 3.2 x 10-3. If the initial concentration of HCl is 0.250 M, what are the equilibrium concentrations of hydrochloric acid, hydrogen gas, and chlorine gas? Show all work. 2HCl(g) ⇄ H2(g) + Cl2(g)
Given the following equilibrium constants at 700K, 2 N2O(g) (double arrow) 2 N2 (g) + O2(g) K1 = 8.2 x 1033NO2(g) (double arrow) 1⁄2 N2(g) + O2(g) K2 = 2.44 x 108N2O4(g) (double arrow) 2 NO2(g) K3 = 4.6 x 10-3 determine the values of the equilibrium constants for the following reaction. Show your equation-buildingprocess and your calculations. 2 N2O4(g) (double arrow) 2 N2O(g) + 3 O2(g) K =
For the equilibrium: Br2(g)+Cl2(g)⇌2BrCl(g) @ 400K, Kc=7.0 Part A: If 0.54 mol of Br2 & 1.23 mol of Cl2Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. Part B: If 0.54 mol of Br2 & 1.23 mol of Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of Cl2? Express your answer to two significant figures and include the appropriate units. Part C: If 0.54 mol of Br2 & 1.23 mol of Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of BrCl? Express your answer to two significant figures and include the appropriate units.
Given the following equilibrium equation and Kc. PF5(g) ⇌ PF3(g) + F2(g) Kc = 2.8 x 10-7 at 30oC If a 0.72 mole sample of PF5(g) is injected into an empty 2.0 liter reaction vessel and the vessel is warmed to 30oC, what is the equilibrium concentration of of PF3(g)? Your answer should have 2 sig figs.
Give typed full explanation not a single word hand written otherwise leave it Determine the equilibrium concentration of D when 6.0 moles of C + 6.0 moles of D in a 2.0L flask 2A(g) + B (g) ←--→ 3C(g) = D (g) Kc = 6.8x10^-6
N2 + 02 > NO for which the equilibrium constant K = 367 at 127 C. Suppose 0.400 mol of N2 and 0.360 mol of 02_ were placed in a 3-liter vessel at 100 C. What will the concentrations of all species be once equilibrium is established?