A chlorine (CI) and bromine (Br) atom are adsorbed on a small patch of surface (see sketch at right). This patch is known to contain 81 possible adsorption sites. The Cl and bromine (Br) atoms have enough energy to move from site to site, so they could be on any two of them. Suppose the Br atom desorbs from the surface and drifts away. Calculate the change in entropy. Round your answer to 2 significant digits, and be sure it has the correct unit symbol. 0 0.0 H 0,0 5 One way a Cl and might be adsorbec surface with 16 sit

A chlorine (CI) and bromine (Br) atom are adsorbed on a small patch of surface (see sketch at right). This patch is known to contain 81 possible adsorption sites. The Cl and bromine (Br) atoms have enough energy to move from site to site, so they could be on any two of them. Suppose the Br atom desorbs from the surface and drifts away. Calculate the change in entropy. Round your answer to 2 significant digits, and be sure it has the correct unit symbol. 0 0.0 H 0,0 5 One way a Cl and might be adsorbec surface with 16 sit

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

Why is kinetic information, in addition to the thermodynamic information provided by enthalpy and entropy, needed to complete our understanding of atmospheric chemistry? Gibbs free energy involves both enthalpy and entropy. Briefly describe the relative roles of the change in enthalpy and entropy in affecting the equilibrium state of a chemical system.
Standard Free Energy of Formation The standard free energy of formation, AG, of a substance is the free energy change for the formation of one mole of the substance from the component elements in their standard states. These values are applicable at 25 °C and are found in thermodynamic tables. The value of AG for a substance gives a measure of the thermodynamic stability with respect to the component elements. Negative values for a formation reaction indicate thermodynamic stability of the product. In other words, the compound formed does not spontaneously decompose back into the component elements. Positive values for a formation reaction indicate thermodynamic instability of the product. Thus, the compound will spontaneously decompose, though the rate may be slow. The sign of AG? can be used to predict the feasibility of synthesizing a substance from its component elements. The standard free energy change for a reaction, AG, is a state function and can be calculated from the standard…
A student dissolves 12.8 g of potassium hydroxide (KOH) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 21.0 °C to 31.9 °C over the course of 7 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: KOH(s) К (ад) + ОН (аq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to 3 significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. exothermic Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ Calculate the reaction enthalpy AH per…
An oxygen (0₂) molecule is adsorbed on a patch of surface (see sketch at right). This patch is known to contain 25 adsorption sites. The (0₂) molecule has enough energy to move from site to site, so it could be on any one of them. Suppose additional surface becomes exposed, so that 225 adsorption sites are now available for the molecule. Calculate the change in entropy. Round your answer to 3 significant digits, and be sure it has the correct unit symbol. 0 ☐ x10 ロ・ロ X μ OO One way an O₂ molecule could be adsorbed on a patch of surface with 16 sites.
Identify whether there will be an increase or a decrease in entropy for the system. Nitrogen gas reacts with hydrogen gas to produce ammonia gas. N2(g) + 3H2(g) → 2 NH3(g) the condensation of steam dry ice subliming magnesium solid reacting with molecular oxygen to produce solid magnesium oxide. 2 Mg(s) + O2(g) → 2 MgO(s)
At SATP, iodine boils at 183.0oC. The vapor pressure of the liquid at 392 K is 0.133 atm. If the molar enthalpy of fusion is 15.65 kJ/mol and the vapor pressure of the solid is 19325 Pa at 38.7oC, calculate its molar enthalpy of vaporization, molar entropy of vaporization and molar enthalpy of sublimation.
What equation should be used to calculate the standard change in entropy for a chemical reaction? (also called the standard reaction entropy)
Calculate the change in entropy round your answer to three significant digits and be sure it has the correct unit symbol
Hi! I'm a college student and i need your help in answering my chemistry subject. Please do help me and I promise to rate it helpful. Please put an understandable or clearer solutions and if possible you can put a brief explanation. Thank you so much and God bless!
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)Mg(�)+Fe2+(��)→Mg2+(��)+Fe(�) at 73 ∘C∘C , where [Fe2+]=3.80mol L−1[Fe2+]=3.80mol L−1 and [Mg2+]=0.210mol L−1[Mg2+]=0.210mol L−1 . What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)Mg(�)+Fe2+(��)→Mg2+(��)+Fe(�) at 73 ∘C∘C when [Fe2+]=3.80mol L−1[Fe2+]=3.80mol L−1 and [Mg2+]=0.210mol L−1[Mg2+]=0.210mol L−1. Assume that the standard cell potential does not depend on temperature. Express your answer to three significant figures and include the appropriate units.
What is the work associated with the decomposition of liquid peroxide forming gaseous oxygen and liquid water at 281.65 K?
3