a cell is roughly spherical with a radius of 25.6 X 10^-6. The surface tension of water is 71.99 mN •m^-1 if the cell grows to double its volume calculate the magnitude of the work required to expand the cell surface. assume the cell is surrounded by pure water and that T= 298. 15K
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- Calculate the difference in slope of the chemical potential against temperature on either side of (a) the normal freezing point of water and (b) the normal boiling point of water. The molar entropy change accompanying fusion is 22.0 J K−1 mol−1 and that accompanying evaporation is 109.9 J K−1 mol−1. (c) By how much does the chemical potential of water supercooled to −5.0 °C exceed that of ice at that temperature?6) A unit cell has the following parameters: a = 5Å b = 10 Å, c =15 Å, a = p = 90°, y = 120°. (i) Determine the parameters of the reciprocal cell. (ii) Find the volume of the real and reciprocal cells, (iii) Find the spacing of the (321) planes. (iv) If Cu Ka radiation is used (X = 1.54 Å) what is the angle of diffraction (20) for the (321) reflection?At room temperature, monoclinic sulfur has the unit-cell dimensions a = 11.04 Å, b = 10.98 Å, c = 10.92 Å, and B = 96.73°. Each cell contains 48 atoms of sulfur. (a) Explain why it is not necessary to give the values of the angles a and y in this cell. (b) Compute the density of monoclinic sulfur (in g cm¯³).
- (b) Using the Crystallographer's formula to determine the density (in g/cm³) of Po: ρ = Σ Ζ * Μ Vell* N You must know that a primitive cubic cell has Z = 1 Since Po is a metal, the value of "i" = 1, since it's the only entity! MM of Po= 208.998 g/mol Vcell (in cm³) = a³ Vcell (3.36 x 10-8 cm)³ = 3.793 x 10-23 cm³ N = 6.022 x 1023 atoms/mol Thus: p = (1 atom/cell) (208.998 g/mol) = 9.16 g/cm³ (3.793 x 10-23 cm³) (6.022 x 1023)5) How many phases are present in the following systems? Also define each of the terminologies associated with the phase diagram. Cu(s) + H2O(g) CuO(s) + H2 (g) NH,C1 NH3 + HCI (3); ZnSO4 . 3H2O(s) + 2H2O(g) (s) (g) ZnSO4. 5H2O(s)Calculate the mass density of diamond assuming that it is a close-packed structure of hard spheres with radii equal to half the carbon–carbon bond length of 154.45 pm. (b) The diamond lattice is in fact based on a face-centred cubic lattice but with two atoms per lattice point, such that the structure consists of two interpenetrating fcc lattices, one with its origin at (0,0,0) and the other with its origin at (1/4,1/4,1/4). The experimentally determined mass density is 3.516 g cm−3: can you explain the difference between this value and that in (a)?
- (a) Magnesium (Mg) has a hexagonal close-packed (HCP) crystal structure with the lattice parameter of a = 0.321 nm and c= 0.521 nm and the atomic radius is 0.173 nm. (i) What is the number of atoms per unit cell in HCP structure? (ii) Determine the atomic packing factor of the Mg unit cell. (iii) Is Mg containing an ideal atomic packing factor? You may justify your answer by evaluating the HCP c/a ratio. Subsequently, will slip be harder in Mg compared to the ideal HCP structure? Justify your answer.Polonium is the only element known to crystallize in the simple cubic lattice. (a) What is the distance between nearest neighbor polo- nium atoms if the first-order diffraction of X-rays with A = 1.785 Å from the parallel faces of its unit cells appears at an angle of 20 = 30.96° from these planes? (b) What is the density of polonium in this crystal (in g cm-3)?For the shown crystal structure, write down (a) the Bravais lattice and (b) the basis of the primitive unit cell. For this structure a=b= c and a=B=y%3D90°. The green (A) atoms at the vertices; blue (B) atom at the center, pink (C) atoms are the centers of two opposite faces; and brown (D) atoms at the centers of four edges of the unit cell. Note that the a, b and c translation vectors are along the positive x, y and z axes, respectively, as shown. COD
- The density of nitrogen at its critical point is 0.3131 gcm-3 . At a very low temperature, 0.3131 g solid nitrogenis sealed into a thick-walled glass tube with a volume of1.000 cm3 . Describe what happens inside the tube as thetube is warmed past the critical temperature, 126.19 K.Determine the enthalpy of vaporization at 343.15 K for water. (Note: The heat of vaporization for water is known to be 40.79 kJ mol-1 at 273.15 K, the Cp of water (Liq) was determined to be 85.6 J K-1 mol-1 and the Cp of water (solid) was to be 54.35 J K-1 mol-1). Use the reaction below and give your final answer in kJ mol-1. H2O(solid, 273.15 K, 0.1 atm)--------H2O(liq, 273.15 K, 0.1 atm)(a) How do the viscosity and surface tension of liquids change as intermolecular forces become stronger? (b) How do the viscosity and surface tension of liquids change as temperature increases? Accounts for these trends