Chapter 23, Problem 11P

(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?

Explain the phase diagram of CaO-MgO.

Using 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 these

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?

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−1

The 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 bonding

If 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. 81833

All 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.

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.