The enthalpy of a simple (and not particularly realistic) model system is given by

H = c1 TP + c2T² /2

where c1 and c2 are constants.

1. Evaluate the partial derivatives (∂H/∂T)_p and (∂H / ∂P)_t . Demonstrate that these partial derivatives satisfy the appropriate Maxwell relations and also determine cP.

2. Construct the inexact differentials (dH)_T, (dH)_P, and the exact differential, dH .

3. Integrate these three differential quantities along the following two paths that connect the same two equilibrium states: (T1, P1) to (T2, P2).

Path 1: The temperature is first increased to T2 at constant pressure, P1. The pressure is then increased to P2 at constant temperature, T2.

Path 2: The pressure is first increased to P2 at constant temperature, T1. The temperature is then increased to T2 at constant pressure, P2.

Compare the integrated values for (ΔH)_T, (ΔH)_P, and ΔH obtained along the two paths.

A mixture containing an initial concentration of 0.1726 M for H2 and 0.1361 M for I2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HI? H2(g) + I2(g) ↔ 2HI(g) Kc = 48.7000

At a temp below room temp but with all components as gases, the decomposition of iodine monochloride, ICl, to iodine and chlorine, is 1.4*10^-5

2ICl (g)----> I2 (g) + Cl2 (g)

If a sealed vessel has [ICl]=1.87 M, and no iodine or chlorine. What are the equilibrium cocentrations?

Calculate the pH of a liter of 0.125 M ammonium perchlorate solution. (kb= 1.7 x 10^-5)

show ice chart!

A window of a car is found to be covered with 0.9cm of ice. If the area of the window is 1 m2, and the ice is at -12 degrees Celsius, what is the minimum heat required to melt all the ice? Take the density of ice to be 900 kg/m3, the specific heat capacity of ice to be 0.5 cal/g*K, and the latent heat of fusion to be 80 cal/g. Answer in kcal.

12. Consider the titration of 0.100 L of 0.200 M ascorbic acid with 0.500 M NaOH. What is the pH at the endpoint of the titration? Enter your answer to two decimal places; for this question we can assume the 5% assumption is valid.

Determine the pH of each of the following solutions.

Part A) 0.25 M KCHO2

Part B) 0.15 M CH3NH3I

Part C) 0.22 M KI

A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was combined with 4.80 mL of 5.90 M NaOH and the resulting solution was diluted to 750 mL. The measured pH of the solution was 4.25.

A student reacts 81g of salicylic acid with 14 mL of acetic anhydride producing 2g of acetyl salicylic acid. What is the percent yield of the reaction?

What mass of ammonium chloride should be added to 2.50 L of a 0.145 M NH3 in order to obtain a buffer with a pH of 9.65?

Determine the pH of each solution.

Dissociation Constants at 25 ∘C

a) 0.21 M KCHO2

b) 0.21 M CH3NH3I

c)0.21 M KI

A battery is constructed from these two half reactions:

            i.   VO²⁺   +   2 H⁺ + e-   → V³⁺   + H₂O        E^o = 0.337 V vs SHE

            ii.   TiF₆^{2 ̶}   +   4 e-   →   Ti(s) + 6 F ^̶                           E^o = ̶ 1.191 V

(a) (0.2 pt) Which half reaction is in the anode compartment?   Circle one:     vanadium rxn      titanium rxn

(b) Which half reaction is in the cathode compartment? Circle one:    vanadium rxn      titanium rxn

(c) Write the balanced chemical equation for the overall battery reaction.

(d) Show the shorthand notation for representing this particular battery:

(e) Calculate the E^o of the battery.

Q: Discuss why matrix effects can be important in AAS.

Q: How can I determine if matrix effects were significant in a sample (let say a tap water).

The osmotic pressure of a solution containing 2.16 g of an unknown compound dissolved in 175.0 mL of solution at 25 ºC is 2.65 atm. The combustion of 25.05 g of the unknown compound produced 58.02 g CO2 and 19.80 g H2O. The compound contains only carbon, hydrogen, and oxygen.

What is the molecular formula of the compound?

Express your answer as a chemical formula

how many ml each are needed to make a buffer with 0.12 M HC3H5O3- (KA=1.4 *10^-4) AND 0.15 NaC3H5O3 that has a pH=3.77