H2 reacts with the halogens (X2) according to the reaction: (8)=x + (8)*H 2 HX(8) where X2 can be Cl2, Br2, or I2. Use the thermodynamic data in Appendix IIB to calculate AH, AS', AG", and K, for the reaction between hydrogen and each of the three halogens. Which reac- tion is most spontaneous? Least spontaneous? What is the main factor responsible for the difference in the spontaneity of the three reactions? Does higher temperature make the reactions more spontaneous or less spontaneous?

H2 reacts with the halogens (X2) according to the reaction: (8)=x + (8)*H 2 HX(8) where X2 can be Cl2, Br2, or I2. Use the thermodynamic data in Appendix IIB to calculate AH, AS', AG", and K, for the reaction between hydrogen and each of the three halogens. Which reac- tion is most spontaneous? Least spontaneous? What is the main factor responsible for the difference in the spontaneity of the three reactions? Does higher temperature make the reactions more spontaneous or less spontaneous?

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

Calculate ΔH°, ΔS° and ΔG° for the synthesis of SO3(g) Be sure to use the values provided in this table: Compound ΔHf° (kJ/mol) S° (J/Kmol) SO2(g) -253 231 SO3(g) -345 219 O2(g) 0 205 a) give the balance equation for the synthesis of SO3(g) from SO2(g) and O2(g) b) What is ΔH° for this process? c) What is ΔS° for this process? d) What is ΔG° for this process?
Using data found in Appendix E of your textbook calculate the nonstandard emf for each of the following reactions if the concentration of each of the lons in these reactions is 0.0003 molar and everything else is standard (use 298 K for the temperature, R = 8.314 J/mol-K, and F = 96,485 C/mol): (a) 1 Sn4+ (aq) + 1 Hg(1) --> 1 Sn²+ (aq) + 1 Hg²+ (aq) (b) 2 Hg2+ (aq) + 1 Co(s) --> 1 Hg₂2+ (aq) + 1 Co²+ (aq) (c) 3 F₂(g) + 2 Cr(s) --> 6 F (aq) + 2 Cr³+ (aq) (d) 1 Ni²+ (aq) + 1 Ca(s) --> 1 NI(s) + 1 Ca²+ (aq) E = E = 11 E = E = V
G.59.
3. Calculate the AH for the reaction C, (graphite) + 2H210) CH, from the following enthalpy changes: Caraphite) + Ozia) Co, AH = -393.5 kJ AH = -571.6 kJ 2H,0 COa + 2H,0 2H, + 0, 2(g) 2(g) CH, + 20, 2(g) AH = -890.4 kJ 4(g) 2(g)
For the reaction CO(g) + Cl₂(g) → COC1₂ (9) ΔΗ° 108 kJ and AS⁰ = – 137 J/K The equilibrium constant for this reaction at 268.0 K is Assume that AH° and ASº are independent of temperature. =
For a certain reaction, AGxn = +3.5 kJ/mol at 298 K. %3! a. If this reaction is at equilibrium, which would you expect to have higher concentra- tions: reactants or products?
1. Given the following reactions and data, use addition (similar to Hess's Law) to calculate AG° for H3PO4 (s). (Hint: The overall reaction is for the formation of 1 mol of H3PO4 (s) from elements in their natural state (elemental phosphorus is P4 (s)). PA () + 5 02@ → P,O10 (5) AG; - 2698 kJ P,O10 (9) + 6 H0 m → 4 H3P04 () H2 ( + ½ 02 (2) → H;O @ AG° = – 396 kJ - 228.6 kJ AG; : AG vap H,O 0 → H2O @ 8.6 kJ Required work: * rewrite the reactions above in the correct direction, using multipliers to change coefficients and modify AG° values if necessary * show that after cancelling, the sum of your reactions gives the desired overall reaction Write the goal equation first?
Carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constant for this reaction using the AG; values in the table. Substance AG; (kJ/mol) H,CO, (aq) -616.1 H, O(1) -237.1 CO,(g) -394.4 K = .002 Carbonic acid then ionizes in water (Kal = 4.5 x 10-7). Ignoring Ka2, estimate K for the overall process by which CO, and H,0 form H* and HCO, . К — Incorrect What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Pco, atm Incorrect
4
Make a non-spontaneous process spontaneous A process that is nonspontaneous can be made spontaneous by coupling it with another process tha is highly spontaneous. The coupling of nonspontaneous reactions with highly spontaneous ones is important in biological system. The oxidization of glucose, for example, is highly spontaneous: C6H12O6(s) + 60₂(g) → 6 CO₂(g) + 6 H₂O(1) Spontaneous reactions such as this ultimately drive the nonspontaneous reactions necessary to sustain life. Can you use Gibbs free energy, enthalpy, and entropy to argue this reaction is highly spontaneous?
Given the dissociation of methane to graphite (C) and hydrogen gas. For the methane at 298K, Given the following data: kJ = -74.85- mol = -80.67 mol · K A,GE.graphite = A,Gån = 0 %3D Solve the following: a. Calculate the equilibrium constant (K) of the dissociation of methane at 298K with the appropriate units. b. Assuming that enthalpy is independent of temperature, Calculate the equilibrium constant (K) of methane dissociation at 1000 K. C. Calculate the ratio between the amounts of methane and hydrogen gas at 298 K and 0.2 bar.
I need the answer as soon as possible