_com/ilm/takeAssignment/takeCovalentActivity.c Use the References to access important values if needed for this question. For the reaction: CH4(g) + H2O(g)3H2(g) + CO(g) AH° = 206 kJ and AS° = 215 J/K The equilibrium constant, K, would be greater than 1 at temperatures Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that AH° and AS° are constant. Submit Answer Retry Entire Group 9 more group attempts remaining

_com/ilm/takeAssignment/takeCovalentActivity.c Use the References to access important values if needed for this question. For the reaction: CH4(g) + H2O(g)3H2(g) + CO(g) AH° = 206 kJ and AS° = 215 J/K The equilibrium constant, K, would be greater than 1 at temperatures Kelvin. Select above or below in the first box and enter the temperature in the second box. Assume that AH° and AS° are constant. Submit Answer Retry Entire Group 9 more group attempts remaining

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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Km.201.
Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
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Consider the following equilibrium: 2NO, (g) – N,04(g) AG = - 5.4 kJ Now suppose a reaction vessel is filled with 7.26 atm of dinitrogen tetroxide (N,O) at 95. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can that yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,0, will tend to fall, can that be changed to a tendency to rise by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it. atm Round your answer to 2 significant digits. O O
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The standard enthalpy of formation of SnCl₂ (s) is - 340 kJ/mol and that for SnCl4 (s) is-511 kJ/mol. From these data, we can calculate that for the reaction SnCl₂ (s) + Cl₂ (g) →→SnCl4 (s), the value of AH O cannot be determined as AH, for Cl₂ (g) is not given. O equals - 851 kJ. O equals + 171 kJ. O equals - 171 kJ.
Problem 10 10 of 12 (> I Review | Constants | Periodic Table MISSED THIS? Watch IWE 18.7; Read Section 18.8. You can click on the Review link to access the section in your e Text. Consider the following reaction: Part A CaCO, (s) + CaO (s) + CO2 (g) 320 K Estimate AG for this reaction at each of the following temperatures (Assume that AH" and AS" do not change too much within the given temperature range.) Express your answer using one decimal place. Πνn ΑΣ φ AG = kJ Submit Request Answer Part B 1080 K Express your answer using one decimal place. AG = kJ Submit Request Answer Part C 1410 K
At -8.64 °C the concentration equilibrium constant K = 7.7 for a certain reaction. Here are some facts about the reaction: -1 • The initial rate of the reaction is 5.3 mol·L¯¹·s¯¹. . If the reaction is run at constant pressure, 132. kJ/mol of heat are absorbed. • The constant pressure molar heat capacity C = 2.97 J'mol K¹. Yes. Using these facts, can you calculate K at 16. °C? x10 O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat 16. °C will be bigger or smaller than K at -8.64 °C? C Yes, and K will be bigger. Yes, and K will be smaller. No.
Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl (aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PbCl2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+: mol/L and Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 10-3 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-³M is kJ/mol. Show your calculations on the separate sheet of paper.
Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g) <-----> 2H2O(g) + 2SO2(g) H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added
[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = -111 kJ/mol, and K. = 0.159 , at 723 K. N2 (g) + 3 H, (g)=2 NH3 (g) When 0.21 moles of NH, (g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish coquilibrium. O remain the same. It is already at cquilibrium. The concentration of H, will Submit Answer Retry Entire Group 1 more group attempt remaining
The system described by the reaction CO (g) + Cl₂ (g) = COC12 (9) is at equilibrium at a given temperature when Pco = 0.28 atm, Pal₂ = 0.12 atm, and Pcoci, = 0.59 atm. An additional pressure of Cl₂ (g) = 0.42 atm is added. Part A Find the pressure of CO when the system returns to equilibrium. Express your answer using two significant figures. IVE ΑΣΦ P = 0.054 Submit Previous Answers Request Answer X Incorrect; Try Again ? atm