Consider the following equilibria: Equilibrium I: H,Og + C - Equilibrium II: Cr2O4 (aq) + 2H“(aq) H2(g) + CO(g); Cr207 (ag) +H2O) AH =+131 kJ mo-1 Use Le Chatelier's principle to predict and explain the effect of: i. increasing the pressure on Equilibrium I. ii. increasing the temperature on Equilibrium I. iii. increasing [H+] on Equilibrium II. iv. the presence of a catalyst on Equilibrium II.

Consider the following equilibria: Equilibrium I: H,Og + C - Equilibrium II: Cr2O4 (aq) + 2H“(aq) H2(g) + CO(g); Cr207 (ag) +H2O) AH =+131 kJ mo-1 Use Le Chatelier's principle to predict and explain the effect of: i. increasing the pressure on Equilibrium I. ii. increasing the temperature on Equilibrium I. iii. increasing [H+] on Equilibrium II. iv. the presence of a catalyst on Equilibrium II.

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

c. In a different equilibrium mixture, under different conditions, the partial pressures of the gases are shown in the table: Gas Partial pressure / kPa N2 1.20 x 102 H2 1.50 x 102 NH3 1.10 x 103 Calculate the value of the equilibrium constant (Kp) for this reaction and give its units. d. The enthalpy change for the reaction is -92 kJ mol-1 State the effect, if any, of an increase in temperature on the value of Kp for this reaction. Explain your answer. 3. a. Name the catalyst used in the Haber process. b. Explain why a catalyst does not change the yield of ammonia produced. c. Sketch a Maxwell Boltzmann distribution curve (with labelled axes) and use it to explain why a catalyst will increase the rate of reaction.
Consider the equilibrium system below for nos. 6 - 9. orations 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(1) AH = -1530.4 kJ How will the amount of ammonia (NH) at equilibrium be affected by: 6. adding O2(g)? no effect 7. adding H20(1)? increase 8. decreasing the temperature? increase 9. decreasing the volume of the container at constant temperature? no effect 11:15 pm 74T Cloudy A ENG
[Review Topics] Use the References to access important v Consider the following system at equilibrium at 1150 K: 2S0,(g) + O2(g)=250;(g) When some O,(g) is removed from the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of SO, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support
Please don't provide handwritten solution ...
7. Ammonia can be synthesized according to the equation: 1/2 N₂(g) + 3/2 H₂(g) → NH3(g). The equilibrium constant is 1.69 x 10-4 at 673 K and AHO is -106.5 kJ mol-¹. Calculate the equilibrium constant at 773 K.
C2. Subject Chemistry
20 <. At a certain temperature, 0.940 mol SO, is placed in a 2.50 L container. 2 SO, (g) =2 SO, (g) + 0,(g) At equilibrium, 0.140 mol O, is present. Calculate Ke. K. = 2.7738 x10-2 Incorrect help about us privacy policy terms of use careers contact us O Bi w
Given the reaction shown below: Colg) + H;0(g) CO,(g) + H2(g) K-0.640 and with the following initial concentrations: (CO)-0.626 M (CO)= 0.981 M [H,O]= 0.5 M [Ha)= 0.95 M Select the statement that best describes the reaction. O The reaction is not at equilibrium. The reaction will shift to the left to reach equilibrium. O The reaction is at equilibrium. It will not shift in either direction. O The reaction is not at equilibrium. The reaction will shift to the right to reach equilibrium. O None of these. O The reaction is not at equilibrium. The reaction will not shift on its own to reach equilibrium.
The chemical equation for an equilibrium is described below. kJ mol CaO (s) + CO2(g) = CaCO3(s) AH° Predict how the following changes would shift the equilibria. Be sure to start by writing the equilibrium (K) equation. =-176-
Given the following initial partial pressures, what is the equilibrium concentration of SO3 (e)? SO2 () + NO2 (s) SO3 () + NO (g) K, = 3.75 (at the current temperature) Initial Species Pgas (atm) SO2 0.277 NO2 0.226 SO3 0.756 NO 0.878 IMPORTANT: When entering your answer: • Enter the number only (no units) Do not leave any spaces • Use a leading zero before the decimal when necessary Report your number to 3 decimal places (regardless of the significant figures) • Correctly round your answer to the 3rd decimal place (allowed margin of error is only ± 0.001, so always use un- rounded numbers in your calculations) Examples: 0.123 or 9.876
Consider the following system at equilibrium where AH° = 18.8 kJ, and K. = 9.52x102, at 350 K: CH4 (g) + CCl, (g) =2 CH,Cl, (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of K. |A. Increases B. Decreases C. Remains the same |A. Is greater than K. B. Is equal to K. C. Is less than K. The value of Qe JA. Run in the forward direction to restablish equilibrium. The reaction must: B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl, will: A. Increase. B. Decrease. C. Remain the same.
For the following equilibrium system, K = 1.39x10-11 at 298 K. F (aq) + H₂O (1) HF (aq) + OH- (aq) Assuming that you start with just F, and that no HF or OH is initially present, which of the following best describes the equilibrium system? O The forward reaction is favored at equilibrium. O The reverse reaction is favored at equilibrium. O Appreciable quantities of all species are present at equilibrium.