Assuming you start with 1 atm of product gas and allow the mixture to reachequilibrium, what will be the mole fraction of product gas for the followingreaction given the Gibbs energy and the temp provided. Assume no quadraticneeded.X(g) +Y(g)<>XY(g)dGrxn--6.9 kJ/molTemp = 264 K0.960.66 margin of error +/- 5%

Answered: Image /qna-images/answer/159cea47-8bda-4ce7-b3bb-efb2b5c08d15.jpg

Answered: Assuming you start with 1 atm of…

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...

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Consider the reaction of N₂O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O₂ and 0.200 mol N₂O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.0100 0.0410 0 -0.0100 0.0710 1 2 N₂O(g) + 3 O₂(g) = 4 NO2(g) 2N₂O(g) 0.0560 -0.0050 0.0360 0.200 0.0050 0.180 + -1.00 0.0150 30₂(g) 2 -0.0560 -0.0150 0.0200 0.210 4NO₂(g) RESET -0.0200 0.190 +
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The equilibrium constant, Kc, for the following reaction is 0.0180 at 698 K. 2HI(g) → H₂(g) + 12 (9) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. HI [H₂] [1₂] = = = M 3 M
For items 10-12. The decomposition of NH4Cl (s) at a given temperature of 548 K, the Kp = 0.01072. NH4Cl (s) = NH4 (g) + HCl (g) 10. If 10.00 g of solid NH4Cl (s) is introduced to the reaction vessel of 500 mL and the system is allowed to reach equilibrium, calculate for the partial pressure of the ammonia. NH4Cl (s) NH4 (g) + HCl (g) C. 0.0212 atm A. 0.104 atm B. 8.41 atm D. 5.30 atm E. 0.00198 atm 11. What is the Kc of the reaction at the given temperature? A. 2.48 x 10-⁹ B. 2.35 x 10-4 C. 1.59 x 10-3 D. 5.16 x 10-6 12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial equilibrium constant. The A,H= 176.01 kJ/mol A. 538 K B. 558 K C. 265 K D. 285 K
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For the reaction A + B --> 2 C, Kç = 0.16. A 2.00 L flask is filled with 1.00 mol A and 1.00 mol B, and allowed to come to equilibrium. Determine the concentrations, in moles/liter, of A, B and C at equilibrium. (Do not input units, 3 sig figs). A = B = C =
Gaseous CH4 and H2O were mixed in a 0.64L flask at 1800K. At equilibrium, the flask contains 0.36 mol of CO, 0.081 mol of H2 and 0.051 mol of CH4 What is the concentration of [H2O] at equilibrium? K = 0.28 for CH4 + H2O -> CO + 3H2
cula... = 18.3 Gibbs Free E... O Kinetics and Equilibrium Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 0.10 mol of Cl₂ and 0.50 mol of HCI. The following reaction becomes possible: H₂(g) + Cl₂(g) -2HCl(g) M 18.3 Gibbs Free E... The equilibrium constant K for this reaction is 0.204 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. Explanation DEC 10 Check 5.3 Enthalpies of... CP 18.5 Gibbs Free E... X tv Nall © 2023 McGraw Hill LLC. All Rights Resea A
Equilibrium Constant, K Test tube 1 = 75.0 Test tube 2 = 88.2 Test tube 3 = 167 Test tube 4 = 161 Test tube 5 = -49.6 For which test tube should your value for the equilibrium constant be most reliable? Justify your selection based on your data and your laboratory experience in completing this procedure.
For the reaction 2 SO,(g) + 0,(g) =2 SO;(g) the equilibrium constant is K. = 15 M-' at 850 K. Three sets of concentrations are given for the three gases in the reaction. For each set, predict the direction in which the net reaction will proceed toward equilibrium. Left No change Right Answer Bank [so,] = 0.20 M [0.] = 0.60 M [so,] = 0.60 M [so,] = 0.72 M [0] = 0.69 M [So,] = 0.63 M [So,] = 0.12 M [0] = 0.12 M so,] = 0.56 M
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