Find the value of the equilibrium constant at 298.15K for the reaction 2SO2(g) +O2(g) = 2SO3(g) b. 0.2000 mol of SO2 and 1.000 mol of O2 are mixed and maintained at a constant total pressure of 1.000 bar and a constant temperature of 298.15K. Find the equilibrium partial pressure of each gas.

Find the value of the equilibrium constant at 298.15K for the reaction 2SO2(g) +O2(g) = 2SO3(g) b. 0.2000 mol of SO2 and 1.000 mol of O2 are mixed and maintained at a constant total pressure of 1.000 bar and a constant temperature of 298.15K. Find the equilibrium partial pressure of each gas.

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

Please write full calculations and explain math At 700 K, the reaction2SO2(g) + O2(g) ⇌ 2SO3(g) has the equilibrium constant K = 4.3 × 106, and the following initial partial pressures present: pSO2 = 0.010 bar; pO2 = 0.010 bar; pSO3 = 10. bar. Calculate Q and predict in what direction the reaction will proceed to reach equilibrium.
Consider the gas-phase reaction for the synthesis of methanol from CO(g) and H₂(g) CO(g) + 2 H₂(0)=CH₂OH(g) The value of the equilibrium constant Kp at 495 K is 1.42 x 10-2. Initially equimolar amounts of CO(g) and H₂(g) are introduced into the reaction vessel. Determine the value of Sea/no at equilibrium at 495 K and 29 bar. X
Consider the following reaction: 2H2O(g) + 2SO2(g) ⇌ 2H2S(g) + 3O2(g) A reaction mixture initially contains 6.2 bar H2O and 4.8 bar SO2. Determine the equilibrium partial pressure of H2S if K for the reaction at this temperature is 1.3 × 10-6 Please explain with full calculations
I am doing a calculation wrong somewhere. It keep getting the wrong answer.
For the following reaction: A(g) + 3 B(g) magnitude of Kp (don't report the units) assuming the following composition at equilibrium: PA = 0.735 bar PB = 0.603 bar Pc = 0.627 bar PD 0.87 bar = 2 C(g) + D(g) Calculate the =
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
Keq for a Gas-Phase Reaction A 5.00-L vessel contained 9.49×102 mol of gaseous PCI3, 8.03×102 mol of gaseous PCI5, and 8.21x102 mol of Cl2 gas at equilibrium at 233°C. Calculate the value of Keg (expressed in terms of the molar concentrations) for the reaction PCI3(g) + Cl2(g) = PCI5(g) (No units required.)
Consider the reaction: Nio (s) + CO (9) = Ni (s) + CO2 (g) K. =4000.0 at 1500 K When calculating the answer, do not round to the appropriate number of significant figures until the last calculation step.
Calculate the reaction quotient, Qr for the following reactions and conditions: 7. 2 SO3(g) 2 SO2(g) + O2(g) 16.5; Pso3 = 0.45 atm; Pso2 = 1.52 atm; : Кр- %3D Po2 = 0.210 atm 8. 2 NO(g) + Cl2(g) → 2 NOCI(g) : Кр- 2.5 x 103; PNo = 0.0032 atm; Pc12 = 0.023 atm; PNOCI = 0.210 atm 9.2 NH3(g) N2(g) + 3H2(g) : Кр- 17.0; PNH3 = 0.13 atm; PN2 = 0.34 atm; |3D PH2 = 1.1 atm %3D 10. Will the system in Question 7 proceed to reactants or products for the conditions given? 11. Will the system in Question 8 proceed to reactants or products for the conditions given? 12. Will the system in Question 9 proceed to reactants or products for the conditions given? 13. For the chemical reaction in Question 7, if it is at equilibrium which direction will it shift if SO2 is added? 14. For the chemical reaction in Question 8, if it is at equilibrium which direction will it shift if NO is removed? 15. For the chemical reaction in Question 9, if it is at equilibrium, which direction will if shift if all the…
Solid NH4I ammonium iodide (which is always considered to be in excess) is introduced into an initially empty container at a constant temperature of 427°C. An equilibrium is quickly established and the total pressure (PT) is then 0.9 bar. NHẠI (s) 2 NH3(g) + HI(g) Express the equilibrium constant K' of this reaction as a function of PT a. Express the equilibrium constant K' of this reaction as a function of PT- The answer is PNH, PHI - - ( 2 2 P K' || po2 p°2 2P°, Can you explain why we get (p/2)^2?