The temperature of a block of copper is increased from T0 to T without any appreciable change in its volume. Show that the change in its specific entropy is

Δs = cp ln (T/T0) - v0β2/κ (T-T0) (equation is attached in a better form)

Δs = change in specific entropy

cp = specific heat at constant pressure = d(bar)q/dT at constant P or partial h/partial T at constant P

κ = isothermal compressibility = -1/v (partial v/partial P)constant T

(T-T0) = final temperature - initial temperature

I know I have to use the second TdS equation (Tds = cp dT - Tvβ dP) and change variable from P to T by using the fact that the volume is constant and expressing dv in terms of T and P.

A one kilogram block of ice melts at 0°C and slowly warms up to the room temperature 30° C.
(a) What is the change in entropy of the ice/water?
Here's what I did:
L_ice = Q/m = 80 cal/g = 80000 cal/1 kg
deltaS_ice = Q/T = (80000)(4.186)/273 = 334880 J/273 K = 1226.67 J/K
L_water = Q/m = 540 cal/1 g = 540000 cal

5.9 Two equal quantities of water, of mass m and at temperatures T1, and T2, are adiabatically mixed together, the pressure remaining constant. Show that the entropy change of the universe is
[see the attachment for the equation]
where c_p, is the specific heat of water at constant pressure. Show that [delta]S >= 0. (Hint: (a

100 g of ice is melted at 0 degree C, and the resulting water is warmed to room temperature (25 degree C). Calculate delta S (change in entropy) for this whole process and comment on the relative magnitude of the entropychanges for the two steps. Explain the sign of delta S.

Using the data sheet (see attachment) calculate delta S values for the following reactions. In each case explain the sign of delta S.
N2H4(g) + H2(g) --> 2NH3(g)
2Al(s) + 3Cl2(g) --> 2AlCl3(g)
Mg[OH]2(s) + 2Hcl(g) --> MgCl2(s) + 2H20(l)
2CH4(g) --> C2H6 + H2(g)

A 40 g block of ice is cooled to -78 degrees C and is then added to 560 g of water in an 80 g copper calorimeter at a temperature of 25 degrees C
Determine the final temperature of the system consisting of the ice, water and calorimeter. If all the ice melts, determine how much ice is left.
Remeber that the ice must fir

1. Define entropy and relate to probability of microstate formation.
2. Relate entropy and reaction spontaneity, Gibbs free energy and reaction spontaneity, and Gibbs free energy and the equilibrium constant of a reaction.
3. Calculate the entropychange within a system and determine absolute entropies.
4. In your own w

ChemLab program "specific heat" lab.
Obtain 100 g shots of each: iron; copper & aluminum. Insert 150 ml of water at room temperature and heat to a
final temperature of 100 degrees of celsius.
Place in calorimeter and add 100 ml of water 20 degrees celsius.
Measure specific heat for each metal and atomic weight.
100

(a) Find the rate of energy flow through a copperblock of cross-sectional area 15 cm^2 and length 8.0 cm when a temperature difference of 30 degree C is established across the block. Repeat the calculation assuming the material is (b) a block of stagnant air with these dimensions; (c) a block of wood with these dimensions.