Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Define isotropy and anisotropy with respect to material properties
For the common allotropes of carbon (graphite and diamond), C(gr) ⟷⟷ C(dia) with equilibrium constant K = 0.32. The molar volumes of graphite and diamond are, respectively, 5.30 cm3/mol and 3.42 cm3/mol; ΔHf of diamond is 1.90 kJ/mol. These data suggest that the formation of diamond is favored at
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low temperatures and high pressures.
high temperatures and high pressures.
low temperatures and low pressures.
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The enthalpy of the fusion of metal Cesium is 13.5 kJ/mol at the melting point of 28.5 oC.Calculate the entropy change for Cesium going from solid to liquor.
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- CacO3(s)C hment/takeCovalentActivity.do?locator%=Dassignment-take [References] Use the References to access important values if needed for this question. For silicon, Si, the heat of fusion at its normal melting point of 1410 °C is 46.4 kJ/mol. The entropy change when 2.12 moles of solid Si melts at 1410 °C, 1 atm is J/K.arrow_forwardCan crystalline silicon become more stable in a reaction that is thermodynamically favoured but kinetically disfavoured? Explain.arrow_forward(a) Given the ionic radii, Cst = 1.67Å, CI = 1.81Å, and the Madelung constant M(CSCI) = 1.763, determine to the best of your ability the molar Crystal energy (AEcryst) for CsCl. (b) Not given additional data, do you expect the value obtained to be larger or smaller than theoretical, and by how many percent do you anticipate to be off?arrow_forward
- The standard free energy of formation of cubic silicon carbide (SiC) is 62.8 kJ mol-1 . Determine the standard free energy change when 1.00 mol SiC reacts with oxygen to form SiO2 (s, quartz) and CO2(g). Is silicon carbide thermodynamically stable in the air at room conditions?arrow_forwardCalculate the delta H for the following balanced equation using the values in the Thermodynamic Properties Table: 2CH3OH(l)+3O2(g)-->2CO2(g)+4H2O(g)arrow_forwardUsing the thermodynamic tables and the enthalpy of formation for one mole of potassium chlorate solid, find the enthalpy change for formation of 15.0 g KClO3 (s) a. – 48.7 kJ b. + 5.97 x 103 kJ c. – 397.7 kJ d. – 3.25 kJ e. – 5.97 x 103 kJ f. none of thesearrow_forward
- Given the information below, calculate the lattice enthalpy for MX(s), where M is a group 1 metal, and X is a group 17 element (standard state: X2(g)). ΔfH°(MX) = -462 kJ mol−1 ΔsubH°(M) = 127 kJ mol−1 D(X2) = 442 kJ mol−1 IE1(M) = 480 kJ mol−1 Eeg1(X) = -142 kJ mol−1 Express your answer to four significant figures. ΔlattH°(MX) = Answer kJ mol−1arrow_forwardExplain the phase diagram of CaO-MgO.arrow_forwardAll compounds in a chemical series have the same commonality of structure, therefore the same predominant IMF. Using concepts of intermolecular forces, please explain thetrends of decreasing ΔTwith increasing molar mass within a chemical series.arrow_forward
- Calculate the standard enthalpy of formation of NaHCO3(s) given the following information:ΔfH°[ CO2(g) ] = −393.41 kJ mol-1, ΔfH° [ NaOH(s) ] = −425.61 kJ mol-1ΔrxnH°[NaOH(s) + CO2(g) ⟶ NaHCO3(s) ] = −127.5 kJ mol-1 Construct a diagram depicting ΔrxnH° of the above reaction and the standard enthalpies of formation of the associated products and reactants.arrow_forwardIf you know that the atomic weight of a metal is 132.9 and its density is 3 gm / cm 1.873 and that each atom of it contributes one electron to the electronic gas. The Fermi temperature of this metal is (in units of K): 1. 58400 2. 100904 3. 70805 4. 81833arrow_forwardThe amount of saturation not only has an effect on the chemical but also the physical properties of the fat. For example, animal fat which is about half saturated and half unsaturated fat is a solid at room temperature but vegetable fat which is about 85 % unsaturated fat is a liquid at room temperature. This is because saturated fats are more linear compared to unsaturated which are nonlinear (bent), meaning that saturated fats are capable of more of what kind of interaction? Hydrogen bonding van der Waals Ionic bonding Covalent bondingarrow_forward
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