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22 Cards in this Set

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Calculate the standard voltage for the reaction:

2Fe+2 (aq) + 2I- (aq) -> 2Fe+2 (aq) + I2 (aq)
E(cell) = .24 V
calculate standards voltages ofr half reactions
Indicate the line notation for this reaction:

3Fe (s) + 2Au+3 -> 3Fe+2 + 2Au (s)
3Fe/3Fe+2//2Au+3/2Au
For this reaction, write the half reaction and calculate the voltage of the cell.

Co/Co+2//Ni+2/Ni
oxid: Ni+2 -> (+2e-) Ni
red: Co -> (-2e-) Co+2

E(cell) = .03V
Find half reactions to find E.
What are the signs of (delta)H and (delta)S for a reaction that:
(a) is spontaneous at all temperatures
(b) becomes spontaneous as temperature increses
(a) (delta)H = (-)
(delta)S = (+)
(b) (delta)H = (-)
(delta)S = (+)
Predict the signs of (delta)S for the following processes:
(a) osmosis
(b) compressing a gas
(c) NO(g) + 1/2 O2(g)->NO2 (g)
(d) precipitation of a solid from a solution
(e) filtration (separation)
(a) (+)
(b) (-)
(c) (-)
(d) (-)
(e) (-)
(delta)S < 0 = low enthalpy (order)
(delta)S > 0 = high enthalpy (disorder)
The autonionization of water at 25*C:
H20 (l) -> H+(aq) + OH-(aq)
has the equilibrium constant 1.0x10-14. Calculate (delta)G* for this process at 25*C.
79.87 J
(delta)G = -RT ln(K)
Balance the equation of the acidic solution.

ClO3- + Fe+2 -> Cl- + Fe+3
ClO3- + 6Fe+2 + 6H+ -> Cl- + 6Fe+3 +3H2O
half reactions
Balance the equation of the acidic solution.

Cu + H+ + NO3- -> Cu+2 + NO +H2O
3Cu + 8H+ + 2NO3- -> 3CU+2 + 2NO + 4H2O
half reactions
Balance the equation of the acidic solution.

MnO4- + H+ + Br- -> Mn+2 + Br2 + H2O
2MnO4- + 16H+ + 10Br- -> 2Mn+2 +5Br2 +8H20
half reactions
Balance the equation of the acidic solution.

Cr2O7-2 + I2 -> Cr+3 + IO3-
5Cr2O7-2 +3I2 +34H+ -> 10Cr+3 + 6IO3- +17H20
half reactions
What is the conentration 9M) of a H2SO4 solution if 18.5mL of acid is required to neutralize 23.4 mL of 0.50 M NaOH?
.315 M ?
2M(A)V(A) = M(B)V(B)
Will a precipitate of lead (II) chloride form when 20.0 mL of 0.38M Pb (NO3)2 and 30.0 mL of 0.18M KCl solutions are mixed. The Ksp of PBCl2 is 1.9x10-4.
Determine [PB+2], [Cl-], [NO3-], and [K+] after the ppt. forms.
Q> Ksp -> precipitate forms
[Cl-] = 0
[Pb+2] =
[NO3-] =
[K+] =
In water, hydrazoic acid, HN3, is a weak acid that has an equilibrium constant, Ka=2.8x10-5 at 25*C. A 0.300 liter sample of a 0.050 M solution of the acid is prepared.
(a) Write the equation for the dissociation reaction.
(b) Write the expression for the equilibrium constant, Ka, for hydrazoic acid.
(c) Calculate the pH of this solution.
(a) HN3 + h2) <-> H3O+ + N3-
(b) Ka = ([H+][N3-])/[HN3] = 2.8x10-5
(c) pH= 3.2?
(a) add water
(b) Ka = [products]/[reactants]
(c) ice box
A 0.100 M solution of the weak acid HX has a pH f 4.50.
(a) Calculate Ka HX.
(b) Calculate the pH of a 0.200 M solution of HX.
(a) Ka = 9.99x10-9
(b) pH = 4.4
(a) find [H+] using pH and set up equilibrium expression.
(b) ice box
Calculate the pH and the percent ionization in the following solution:

0.10 M hydroxylamine (HONH2), Kb = 1.1x10-8
% ionization = .03%
pH = 9.5
ice box
Calculate the pH of a 5.0 M H3PO4 solution. The following information should be useful:
Ka1= 7.5x10-3
Ka2= 6.2x10-8
Ka3= 4.8x10-13
pH = 0.72
make 3 ice boxes
Give the conjugate base of each of the following proton sources.
(a) H3PO4
(b) HBr
(c) HS-
(d) NH4+
(e) PH3
(a) H2PO4-
(b) Br-
(c) S-2
(d) NH3
(e) PH2-
Give the conjugate acid o each of the following bases"
(a) NH3
(b) br-
(c) NH2
(d) H2PO4-
(e) OH-
(a) NH4+
(b) HBr
(c) NH3+
(d) H3PO4
(e) H2O
Consider the system:
2H2S(g) + 3)2(g) <-> 2H2)(g) + 2SO2(g)
(delta) H for the forward reaction in -1036kJ. Predict whether the forward or reverse reaction will occur when the equilibrium is bisturbed by:
(a) expanding the container at constant temperature
(b) removing SO2
(c) raising the temperature
(d) adding water vapor to the system
(a) <p, >V reverse
(b) forward
(c) reverse
(d) reverse
use the pile method
Given:
NOBr(g) <-> NO(g) + 1/2 Br2(g) Keq = 0.71
2N2O(g) + 3)2(g) <-> 2N2O4(g) Keq = 1x106
Calculate keq for
(a) 3NOBr(g) <-> 3NO(g) + 3/2 Br2(g)
(b) N2O4(g) <-> N2O(g) + 3/2 O2(g)
(a) K3
(b) 1/(square root of)K
Consider the reaction :
PCl5(g) <-> PCl3(g) + Cl2(g) K= 5.0x10-4
In an experiment, 0.200 mol of PCl5, 0.500 mol of PCl3, and 0.300 mol of Cl2 are mixed in a 2.00 L vessel. Calculate the equilibrium concentrations of reactants and products.
[PCl5] =
[PCl3] = .1 M
[Cl2] = 0 M
ice box
For a certain first order reaction, A --> products, at 15*C, k = 0.052/hour.
Calculate:
(a) the rate when the concentration of reactant is 0.10M
(b) the half life
(c) the time required for the concentration to drop to 80% of its original value.
(d) What is k at 30*C if the activation energy is 29.0kJ?
(a) rate = .0052/hr.
(b) t1/2 = 13.33hr.
(c) t = 4.29 hr.
(d)
rate = []K
t1/2 = .693/k
t= (ln (100/percentage))/K
hasselback equation