12st woll ooalfit 16 llsw sdi abiewol bodzuggoiad ai bns vewe ji 01 villeitini zi cmoltod sdTSopa Sl afin gaivom qot sdt eiDunLer 10.0nnillsw ztuse12 G (oL )U Un oLE LAoboobjetovlor bas oiitsup wond ni gul 3o noiuonul notaunooftib uovbs ai) noilsita91tib tisilqmi gruzu i of 1ooqa21 di w otunasflib bnsetrvob sin Witiinaup meolmLrITworol tinsbi bns Sunoin dotoesin bainlasATAGL 15.217. Calculate K, for H,O(g) +5 0,(g) = H,0,(g) at 600 K, using the following data:H,(g) + O,(g) P H,0,(g) K, = 2.3 × 106 at 600 K%3D2H,(g) + O,(g) 2H,0(g)= 1.8 x 1037 at 600 Ka) 4.4 x 1043b) 9.8 x 10241.2 x 10-4c)d) 5.4 x 10-13e)2.6 x 10-31ANS: d) 5.4 × 10-13PAGE: 13.2,3

1. When a reaction is multiplied or divided by some number, Kp changes accordingly as follows: A + B…

TAGL 5.4 . Calculate K, for H,O(g) + 5 0,(g) = H,O,(g) at 600 K, using the following data: H,(g) + O,(g) P H,0;(g) K, = 2.3 × 106 at 600K 2H,(g) + O,(g) 2H,0(g) K, = 1.8 × 107 at 600 K a) 4.4 x 1043 b) 9.8 × 1024 c) 1.2 x 10-4 d) 5.4 x 10-13 e) 2.6 x 10-31

TAGL 5.4 . Calculate K, for H,O(g) + 5 0,(g) = H,O,(g) at 600 K, using the following data: H,(g) + O,(g) P H,0;(g) K, = 2.3 × 106 at 600K 2H,(g) + O,(g) 2H,0(g) K, = 1.8 × 107 at 600 K a) 4.4 x 1043 b) 9.8 × 1024 c) 1.2 x 10-4 d) 5.4 x 10-13 e) 2.6 x 10-31

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

For the system ΔΗ = -9.4 kJ H₂(g) + 2(g) 2HI(g) K = 62.5 at 800 K. "Predict the direction of the shift of the equilibrium position at 600 K."
Please don't provide handwritten solution ....
Consider the equilibrium system described be the chemical reaction below, which has a value of Kc equal to 4.10x10-4 at a high temperature. If 0.20 mol N2 and 0.15 mol of O2 react in a 1.0 L vessel, what will the equilibrium concentration of O2 be and set up the expression for Qc and Kc. The reaction is N2 (g) + O2(g) -> 2NO (g)
Consider the following reaction:CH3OH(g) CH2O(g) + H2(g) K = 3.29 x 10−11a. If 14.4 g of CH3OH(g) is added to a 1.50 L container at 298 K, calculate the equilibriumconcentrations of all gases b. Without doing any calculations, predict what happens if the reaction is put in a 2.00 Lcontainer instead of a 1.50 L container. c. . Without doing any calculations, predict what happens if H2SO4 (a catalyst) is added
Consider the reaction: 2 NH3(g) = N₂(g) + 3 H₂(g). At T = 740 K, the equilibrium constant K for this reaction is K₂ = 10. 22. What is the correct form of the equilibrium constant K for this reaction? (A) Kc = (B) Kc = (C) Kc = 2[NH3] [N₂] + 3[H₂] (D) Kc = (E) Kc = [N₂][H₂]³ [N₂] + 3[H₂] 2[NH3] [NH3]² [N₂] [H₂] 3³ 3 [N₂] [H₂]³ 2 [NH3]²
- Calculate the value of the equilibrium constant, K., for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Kc = M(g) Z(g) 6R(g) 2N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kel = 3.85 K2 = 0.570 K3 = 13.2
Considering the following problem, What is the value of the equilbrium constant in terms of concentrations, Kc, at 504.1 K?
At a particular temperature the equilibrium constant K = 2.50 for the following reaction in the gas phase: SO2(g) + NO2(g) = SO3(g) + NO(g). Calculate the equilibrium pressure of SO3(g) in the reaction if the initial pressures of SO2(g) and NO2(g) were both 1.00 bar. and no products had been formed. O 0.20 bar 0.39 bar 1.39 bar 0.61 bar 1.61 bar
For the reaction 2CH4 (g) = C2H2(g) + 3H2(g) K. = 0.140 at 1756 °C.What is K, for the reaction at this temperature? %3D Express your answer numerically.
2NO2(8) 7 N204(g)Kc = 20.0 at 55 \deg CAt 55 \deg C a flask contains 0.040 mol-L-1 NO2(g) and 0.040 mol - L-\ N 204(g). When equilibrium is reached, (A) some of the NO2(g) will have been converted to N204(8). (B)some of the N 204(g) will have been converted to NO2(g). (C) the concentrations will remain at 0.040 mol-L-1 forN02(8) and 0.040 mol-L-1 for N204(8). (D) all of the NO2(g) will have been converted to N204(g).
At a certain temperature, 0.350 mol CH, and 0.676 mol H, S are placed in a 2.50 L container. CH, (g) + 2 H, S(g) = CS,(g) + 4H, (g) At equilibrium, 10.4 g CS, is present. Calculate K.. 0.0574 K. Incorrect
6B.4(b) The equilibrium constant for the reaction N2(g) + O2(g)=2 NO(g) is 1.69×10-3 at 2300 K. A mixture consisting of 5.0 g of nitrogen and 2.0 g of oxygen in a container of volume 1.0 dm³ is heated to 2300 K and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.20