n 14 ch of the following corresponds to a layer of ions unaffected by fluid motion and is separated from the rest of the continuous phase? Stern layer Surface charge Shear plane Diffuse layer
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- Examine the nanoscale diagrams and the phase diagram for Question 112. Match each particulate diagram (1 through 7) to its corresponding point (A through H) on the phase diagram.Which solid phase that is, which allotrope of carbon is more stable, graphite or diamond? You should consult some of the tables in the thermodynamics section of this text.. Both solid phases exist under normal conditions of pressure and temperature. Explain why this is so, given that one solid phase is more thermodynamically stable than the other. Do their unit cells provide any suggestion for their relative stabilities?1. For coexistence curves in a phase diagram for a typical pure substance, which is more sensitive to pressure: boiling point or melting point? (a) boiling point (b) melting point TI
- The smectic liquid crystalline phase can be said to be morehighly ordered than the nematic phase. In what sense isthis true?Barium titanate (BaTiO3) is an ionic solid with a density of 6.02 g/cm3. Its structure is described by orthogonal basis vectors (i.e. at 90 degrees to each other) with lattice parameters of a = b = 0.3992 nm and c = 0.4036 nm.a) What crystal system does barium titanate belong to, based on the above information?Explain your answer. b) Find the number of Ba, O, and Ti atoms per cubic centimeter in barium titanate (i.e.provide a value for each element). c) Sketch and label the (111) plane of BaTiO3 with its atoms and dimensions.AH vap In(Pvap) R The following graph was obtained for a pure volatile liquid substance. In(Pvap) 4 3 2 -1 -2 -3 -4 == ²( ) + C 0.002 (Note that Pvap is the vapour pressure in atm.) 1/T (K-¹) Determine the enthalpy of vaporization for this substance. Hvap 0.003
- (f) There are 7 crystal systems, 2 of them are predominant in metals, which are the two?What's More Activity 1. Interpretation of Water and Carbon Dioxide Phase Diagram Liquid Liquid Sold Sele 273 273.2 373 647 2166 Temperatue Temperature ( Phase Diagram of water Phase Diagram of Carbon Dioxide Based on the phase diagrams of water and carbon dioxide, answer the following questions and justify your answers: 1. You have ice at 263 K (-10.0 °C) and 1.0 atm. What could you do to make the ice sublime? 2. A sample of dry ice (solid CO2) is cooled to 173 K (-100.0 °C) and is set on a table at room temperature (298 K; 25 °C). At what temperature is the rate of sublimation and deposition the same (assume that pressure is held constant at 1 atm)?Question 4 Calculate the change in freezing point of water, with ethalpy of fusion = 6.009 kJ/mole) and the density of ice is 0.9167 g/cc while for that liquid is 0.9999 g/cc for an increase in pressure of 1.00 atm at 273 K. Use the editor to format your answer
- Silicon (Si) has the diamond and GaAs has the zinc blende crystal structures. Given the lattice parameters of Si and GaAs, a = 0.543 nm and a = 0.565 nm, respectively, and the atomic masses of Si, Ga and As as 28.08 g/mol, 69.73 g/mol and 74.92 g/mol, respectively, calculate the density of Si and GaAs. What is the atomic concentration (atoms per unit volume) in each crystal?3-The phase diagram below is for a pure substance. Explain what is wrong with phase diagram aFor most substances, the solid is more dense than the liquid. Sketch the phase diagram for such a substance, being sure to have the solid-liquid equilibrium line slope in the correct direction. Use Le Châtelier's principle to explain why the melting point of such a substance should increase with pressure. Select all that apply. O An decrease in pressure should favor the system with the lower volume, i.e. the solid. O If melting were to be accomplished at the lower pressure, it would require a temperature that is higher than the normal melting temperature. O An increase in pressure should favor the system with the lower volume, i.e. the solid. O If melting were to be accomplished at the higher pressure, it would require a temperature that is higher than the normal melting temperature. O If the substance is at its melting point at a pressure of one atmosphere, and then if the pressure were to be decreased, more solid would form at the expense of liquid - that is, more of the substance…