Predicting whether a precipitate forms based on the solubility product and concentrations.

Describe how you would predict whether a precipitate will form when two solutions are mixed. Start with the minimum information needed and then show how you would make the prediction. Assume a constant temperature of 298 K and that the volumes of the two solutions are additive.

eigenfunctions

a) Show that Y20 is not an Eigenfunction of Lx. b) Show that Y00 is an Eigenfunction of Lx. the numbers after the y is a subscript

average values ?

Complete this equation: Lz3 Yl,m = ? Find the following: for the 2p0 for the 2p1

more p-chem

Explain why each of the following integrals must be 0 when the functions are hydrogen -like wavefunctions: <2p1|Lz|3p-1> and <2p0|Lz|2p0> Show that taking the lithium spin orbitals in a Slater determinant as 1sa, 1sb, and 1s(c1a+c2b) where c1 and c2 are constants gives a wavefunction that equals zero. the a and b are alpha a ...continues

p-chem

I asked this question before and was told there wasnt a 2p0 orbital need clarification Find the following: for the 2p0 for the 2p1

energy levels particle in a box

1. If the position of the one dimensional particle in a box relative to the origin of the coordinate sysytem is changed, the energies do not change but the wavefunctions do. Suppose the ends of the box are located at x=-L/2 and x=L/2. Find the wavefunctions for the four lowest energy levels. 2. Complete this equation: Lz3 Y ...continues

Understanding the ideal gas law. Using the ideal gas law to calculate work done as a result of a chemical reaction that generates a gas.

Calculate the work done when 50 g of iron dissolves in hydrochloric acid in (a) a closed vessel and (b) an open beaker. Hint: Use the ideal gas law and equations to determine amount of work done when a gas expands.

Understanding the properties of gases. Understanding partial pressure of a gas in a mixture, and how partial pressure relates to the mole fraction.

One mole of nitrogen and three moles of hydrogen are injected into a container of volume 10 dm^3 at 298 K. What are the partial pressures and the total pressure? (Note: "^" means "to the exponent".)

Understanding "equation of state" (ie. PV=nRT) for an ideal gas, and using equation of state to predict changes in pressure, volume, and temperature.

In an industrial process, nitrogen has to be heated to 500 K in a vessel of constant volume. If it enters the vessel at a pressure of 100 atm and a temperature of 300 K, what pressure does it exert at the working temperature?

Understanding how a real gas (eg. van der Waals gas) differs from an ideal gas. Interpreting the pressure-volume behaviour of gases.

In an industrial process, nitrogen has to be heated to 500K at constant volume. If it enters the system at 300 K and 100 atm, what pressure does it exert at its final working temperature? Treat it as a van der Waals gas. Assume the volume is 1 m^3 (where "^" means "to the exponent").