A chlorine (Cl) atom is adsorbed on a small patch of surface (see sketch at right). This patch is known to contain 16 possible adsorption sites. The Cl atom has enough energy to move from site to site, so it could be on any one of them. Suppose a Br atom also becomes adsorbed onto the surface. Calculate the change in entropy. Round your answer to 2 significant digits, and be sure it has the correct unit symbol. One way a Cl atom might be adsorbed on a surface with 16 sites.

A chlorine (Cl) atom is adsorbed on a small patch of surface (see sketch at right). This patch is known to contain 16 possible adsorption sites. The Cl atom has enough energy to move from site to site, so it could be on any one of them. Suppose a Br atom also becomes adsorbed onto the surface. Calculate the change in entropy. Round your answer to 2 significant digits, and be sure it has the correct unit symbol. One way a Cl atom might be adsorbed on a surface with 16 sites.

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

MUST ANSWER ALL
Acetylene gas, C2H21g2, is used in welding. What is the maximum amount of useful work that can be accomplished under standard conditions by this reaction?
Please help me answer these subunits!
19. Solid urea, (NH2)2CO, burns to give CO2, N2, and liquid H2O. Its heat of combustion is -632.2 kJ/mol. 1.Write the balanced combustion equation. Record fractions as ratios (e.g. 1/2) if needed. Include aggregation states in your answer. 2.Calculate the heat generated per mole of H2O formed to 0.1 kJ. 3.Using this heat of combustion and the appropriate thermodynamic data, determine the heat of formation of urea to 0.1 kJ.
The standard reaction free energy AGO = − 1378. kJ for this reaction: 2 CH3OH(g) + 3O₂(g) →2 CO₂(g) + 4H₂O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. 2 4 ²-CH₂OH(g) + O₂(g) → ²-CO₂(g) + H₂O(g) 3 2 3 reaction 3 -- CO₂(g) + H₂O(g) + H₂O(g) → 2 2CO₂(g) + 4H₂O(g) 1 2 3 CH₂OH(g) + ²/0₂(g) 4 2 2CH₂OH(g) + 30₂ (8) 2 0 46° kJ KJ kJ x10 Ś
The standard heat of reaction for the production of formaldehyde in the reaction, 2 CH;OH (1) + 0: (3) →2 HCHO (g) + 2 H20 (1), is -326.2 k]/mol. a. Is the reaction exothermic or endothermic? Would you heat or cool the reactor to keep the temperature constant? b. Explain physically why heat is released or absorbed when a reaction occurs. c. If the temperature and pressure are keep at standard (25°C, 1 atm), what is the rate of heating/cooling required in kcal/hr if 1000 kg/hr of formaldehyde is formed?
2. Suppose you performed a similar experiment using an unknown sample of carbonate. The pressure and volume were measured after the temperature stabilized at 21.5 °C. Given the data in the table below, what is the stoichiometric ratio between HCl(aq) and CO2(g)? Metal carbonate + HCl(aq) = Metal chloride + CO2(g) + H2O(1) Initial pressure (atm) 1.0 Initial gas volume (mL) 240.0 Volume of 1.0 M HCl solution added to fully consume the carbonate sample (mL) 22.0 Final pressure (atm) 2.32 Final gas volume (mL) 218.0
Ethylene (C2H4) plays an important role in the ripening of certain fruits and vegetables. It is sometimes supplemented under controlled conditions at produce—processing facilities but is also produced naturally by many fruit-bearing plants. Although the actual process by which plants produce ethylene is a complex one, imagine that it is produced by the simple breakdown of glucose according to the equation: C6H12O6 (s) à 3 C2H4 (g) + 3 O2 (g) Given S°= 212.1 J/molK, DG°= -910.56 kJ/mol and DH°= -1274.5 kJ/mol for C6H12O6 (s). a.) Determine the sign of DS° for the reaction. b.) Calculate DS° for the reaction. c.) Using the tabulated DG° values in the appendix, calculate DG° for the reaction. d.) Above what temperature (in °C) is the reaction spontaneous? Hint: you will first have to calculate DH° using tabulated values.
When delta G is zero, the forward and reverse driving forces are equal, and the process occurs in both directions at the same rate. This is referred to as which of the following terms? O standard free energy formation Entropy O Equilibrium O Gibbs free energy change
1. Polymerization reactions are complicated somewhat because they involve very large numbers of molecules. But we can demonstrate the general features of the thermodynamics of polymerization by considering a much smaller model system. Instead of considering the formation of polyethylene, for example, we can begin with the following reaction in which two ethylene molecules combine with hydrogen to form butane: 2 C2H4 + H2g → GH10) Use the table below to calculate ASº. Compound (J mol" K') Compound U mol" K') 130.6 CO:(g) 213.6 O:(g) 205.0 C,H(g) 310.03 II,O() CI L(g) 69.91 186.2 I1,0(g) 188.7 CIL(E) 219.5 NH(g) 1923 C,H,N(O 178.91
6. In a study of glass etching, a chemist examines the reaction between sand (SiO₂) and hydrogen fluoride at 150°C: SiO₂ (s) + 4HF(g) SiF4(g) + 2H₂O(g) Predict the effect on [SiF4] when (a) H₂O(g) is removed; (b) some liquid water is added; (c) HF is removed; (d) some sand is removed.
Calculate AG for this reaction at 25 °C. 3NO2 (g) + H₂O (1)→ 2HNO3(aq) + NO (g) 5 ΑΣΦ ***** 1) ? Pand AG = kJ You have already submitted this answer. Enter a new answer.