For each of the following a-d write the balanced equation including physical sta

ID: 994706 • Letter: F

Question

For each of the following a-d write the balanced equation including physical states, write the expression for the equilibrium constant, K_eq, identify the type of equilibrium constant that is represented. Dissolving calcium phosphate in water: The dissociation of acetic acid in water. The reaction of ammonia with water. The oxidation of chromium metal to chromium (III) by zinc (II). A solution made from adding CH3COONa (s) to an aqueous CH3COOH solution. How would you calculate the change in free energy at 25 degree C for any of the above if given the value of K_eq? What is the value of K_p for water boiling at 100 degree C? Write the chemical equation for the standard formation of solid calcium phosphate, What is the standard change in free energy, Delta G_f degree, of each reactant? For each solution below, predict if the pH that will be above 7, below 7, or approx. 7. What are the units for the rate constants of zero-order, first-order, and second-order reactions? What would be the units of the rate constant of a third-order reaction? Define reaction quotient. How does it differ from equilibrium constant? How can a quotient be used to determine the direction a reaction will proceed? Ethanol has the following melting and boiling points: mp. = -114 degree C & bp. = 78 degree C. What is the most stable physical Mate (or ethanol at room temperature? (solid, liquid. or gas) Predict the signs of DeltaG, DeltaH, DeltaS for the following processes:

Explanation / Answer

1a) Acetic acid= CH3COOH

CH3COOH(aq) + H2O(l) ----> CH3COO-(aq) + H3O+(aq)

This is an acid-base reaction.

Keq= Ka = [H3O+][CH3COO-]/[CH3COOH]

1b) NH3= ammonia

NH3(aq) + H2O(l) ------> NH4+(aq) + OH-(aq)

Is an acid-base reaction, but this time the equilibrium constant is Kb because NH3 is a base.

Keq=Kb= [NH4+][OH-]/[NH3]

1c) This is a redox reaction, we need to write the half reactions and then the overall reaction:

half reactions:

(Cr (s) ------> Cr+3(aq) + 3e-) x2

(Zn+2(aq) + 2e- -------> Zn(s)) x3

---------------------------------------

2Cr(s) + 3 Zn+2(aq) -----> 2Cr+3(aq) + 3Zn(s)

Solids and liquids are not included in Keq.

K= [Cr+3]2/[Zn+2]3

1d) when you add CH3COONa to CH3COOH you are adding CH3COO- ions to the solution, but the Keq is the same as the first one, the only thing that changes is the value of the concentration of the ions.

Ka= [H3O+][CH3COO-]/[CH3COOH]

(Maybe i dont fully understand this part, sorry if it is not correct)

1e) DG is the change in free energy, it is calculated by : DG=DG0 + RTLnQ

DG0 is the change in standard free energy and is calculated by: DG0= -RTLnKeq

So, if we have the values of Keq for the reactions we can find DG0 and then with the concentration of the ions in each case we can find Q (reaction quotient) and finallt find DG.

1f) the reaction is:

H2O(l) <------> H2O(g)

Kp= PH2O = 760 mmHg= 1 atm ----> Kp =1

3a) H2SO3 is a weak acid, so the pH will be lower than 7.

3b) NH4Cl is a salt so it will dissociate in NH4+ and Cl-. The Cl- is the conjugate base of a strong acid, so it will no affect pH. But NH4+ is the conjugate acid of a weak base so, it will modify the pH reacting with water:

NH4+ + H2O <-------> NH3 + H3O+

This reaction generates H3O+ so the pH of the final solution will be under 7.

3c) The CH3NH2 is a base so it will react with water producing OH- ions, the solution pH will be above 7.

CH3NH2 + H2O <------> CH3NH3+ + OH-

3d) NaNO3 is a salt, it will produce Na+ and NO3- . The Na+ is the conjugate acid of a strong base, it will not affect pH, and the NO3- is the conujgate base of a strong acid, so it will not affect pH either. In this case pH is close to 7.

3e) This compound will prodece Na+ (we know it will not affect) and HCOO-. The HCOO- is the conjugate base of a carboxylic acid, wich is weak, so it will modify the pH:

HCOO- + H2O <-------> HCOOH + OH-

pH>7

3f) KNO2 produces K+ and NO2-. K+ is the conjugate acid of a strong base so it will not affect pH, and NO2- is the conjugate base of a weak acid so, it will affect pH:

NO2- + H2O <-----> HNO2 + OH-

pH>7

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