Lauric acid, the major component of virgin coconut oil, is a carboxylic acid whose condensed structural formula is CH3(CH2)10COOH. That is, it is a carboxylic acid that has a 12-carbon hydrocarbon chain. Lauric acid molecules when dispersed in water would tend to primarily because that . O aggregate; would decrease the entropy of decane molecules O aggregate; would increase the entropy of water molecules O separate; would increase the entropy of decane molecules O separate; would decrease the entropy of water molecules

Lauric acid, the major component of virgin coconut oil, is a carboxylic acid whose condensed structural formula is CH3(CH2)10COOH. That is, it is a carboxylic acid that has a 12-carbon hydrocarbon chain. Lauric acid molecules when dispersed in water would tend to primarily because that . O aggregate; would decrease the entropy of decane molecules O aggregate; would increase the entropy of water molecules O separate; would increase the entropy of decane molecules O separate; would decrease the entropy of water molecules

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

For each of the following changes, do you expect the entropy to increase or decrease? (These questions do not require calculations.) a. Ammonia gas and hydrogen chloride gas react to deposit solid ammonium chloride on a surface b. Two aqueous solutions are combined to form a precipitate c. Methanol gas condenses to form liquid methanol d. Butane liquid reacts with oxygen gas to form carbon dioxide gas and gaseous water e. Liquid water freezes to form ice f. Solid lead melts g. A solid solute dissolves in a liquid solvent h. Liquid water boils Possible answers: 1. Entropy should increase (more positive) 2. Entropy should decrease (more negative) 3. The change in entropy cannot be determined from the information given
A Moving to another question will save this response. Question 11 A reaction has an equilibrium constant (K) of 58.2. If the entropy of this reaction is-36.7 J/mol"K at a temperature of 317 K, what is the enthalpy of this reaction in kJ/mol? Report your answer to one decimal place. If your answer is negative, make sure to input a negative sign (-). Moving to another question wvill save this response. lyp 144 &
Which of the givenn processes will cause a decrease in entropy? Note only one is correct. - dissolving NaCl in water? - removing a partition to mix two gases? - freezing water to make ice? - boiling water to make steam? - heating ice to make water?
REFER TO IMAGE
Which of the following processes will result in an increase in entropy for the system? (A) 2N2O(g) + O2(g) --> 4NO(g); (B) 2NO(g) + O2(g) --> 2NO2(g); (C) CO(g) + NO2(g) --> CO2(g) + NO(g); (D) SO3(g) + H2O(l) --> H2SO4(aq)
Compare what will happen to the entropy of the whole system in the following two scenarios: A) if the oil molecules are all clumped together and the clump is surrounded by water and B) if the oil molecules are spread out evenly throughout the water, each individual oil molecule surrounded by water?
At 0.9 bar of pressure and 373.15 K, the hypothetical transition from liquid to gaseous water will result in what change in the total entropy of the “universe”? No change An increase in the total entropy A decrease in the total entropy Not enough information to determine
Spontaneous chemical reactions proceed until they hit equilibrium. Once the reaction hits equilibrium, it stops until the product or reactant concentration changes. The reaction will then start again until the equilibrium concentrations of reactants and products are restored. If the statement isn’t accurate then tell me why that is the case.
1. In different phases of water, this has the highest entropy because molecules are too farapart to form H-bonds and they can move freely in any direction.