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Thermodynamics and Energy
Rate Laws
Equillibrium
Acid & Base Reactions
Electrochemistry
100

The values of ΔG that a reaction is spontaneous

What are negatives

100

The rate of appearance of 2F- (aq) given the rate of appearance of Ca2+ (aq) is 0.57 mol/sec and the equation:

CaF2 (s) <--> Ca2+ (aq) + 2F- (aq)

What is 1.14 mol/sec?

100

The elemental states that are included in an equilibrium expression

What is aqueous and gaseous

100

Find pH of 0.2 M CH3NH3I (Ka = 2.27 x 10-11).

What is 5.67?

100

The half-reactions in the following reaction, labeled as oxidation and reduction:

Fe3+ (aq) + Cu2+ (aq) --> Cu (s) + Fe2+ (aq)

What is - 

Oxidation: Cu2+ (aq) + 2e- --> Cu (s)

Reduction: Fe3+ (aq) + e- --> Fe2+ (aq)

200

Heat is a product in this type of reaction

What is exothermic

200

The y-axis scales that give the zero, first, and second-order graphs a linear relationship

What is [A], ln[A], and 1/[A], respectively

200

The equilibrium concentration of [NO3] given the following reaction with a Ksp of 1.56 * 10-2 


What is 0.125 M [NaNO3]

200

All Strong Bases and Acids

What is

Acids:

HCl, HBr, H2SO4, HNO3, HI, HClO4

Bases:
LiOH, NaOH, KOH

200

The Eocell of the following reaction and whether or not it is spontaneous:

Zn2+ (aq) + Cu (s) --> Cu2+ (aq) + Zn (s)

What is -1.10 V, Nonspontaneous

300

The ΔGo for the following equation at 25oC:

C2H5OH (l) + 3O2 (g) --> 2CO2 (g) + 3H2O (g)

Compound   ΔGfo (kJ/mol)  
C2H5OH (l)         -910              
O2 (g)                  0            
CO2 (g)            -394          
H2O (g)             -229              

What is -1300 kJ/mol

300

The order of A if it doubles between rates

Rate1 = 0.00448

Rate2 = 0.01792

What is second-order?

300

The equilibrium expression for the following reaction

CaCl2 (aq) + Na2CO3 (aq) <--> CaCO3 (s) + 2NaCl (aq)

What is [CaCl2][Na2CO3]/[NaCl]2

300

The pH of a solution containing 150 mL of 2.7 M NH3 (Kb = 1.8 * 10-5).

What is 11.84?

300

Find the E cell:

Co2+ (aq) + Sn (s) --> Sn3+ (aq) + Cr (s)

What is -0.140 V?

400

Which of the following is not a spontaneous process at room temperature? 

a) sugar dissolves in water

b) melting of iron

c) rusting of iron

d) evaporation of water

What is melting iron?

400

Determine the rate law for the reaction

S2O82- (aq) +3I- (aq) -> 2SO42- (aq) + I3 (aq)

Rxn    [S2O82]     [I-]       Inital Rate (M/s)

1          0.67      0.42        36.2

2          0.44      0.42        23.8

3          0.44       0.21        11.9

What is

Rate = 128.6 M-1s-2 [S2O82][I-] 

400

The equilibrium constant for the following reaction:

N2 (g) + 2O2 (g) <--> 2NO2 (g)

[N2] = 0.150 M
[O2] = 0.100 M
[NO2] = 0.050 M

What is Kc = 1.67

400

A 25.0 ml of solution of 0.1 M HOCl is titrated with a 0.2 M NaOH soln (Ka HOCl = 4.0 x 10-8). Calc pH when 8.5 ml of NaOH was added.

What is 7.73?

400

The following redox reaction balanced in basic solution:

MnO4- (aq) + Co (s) --> Mn2+ (aq) + Co2+ (aq)

What is

8H2O (l) + 2MnO4- (aq) + 5Co2+ -->

2Mn2+ (aq) + 5Co (s) + 16OH- (aq)

500

The ΔGo for the following equation at 25oC:

SiO2 (s) + 4HF (g) --> SiF4 (g) + 2H2O (g)

Compound   ΔHfo (kJ/mol)  So (J/mol)
SiO2 (s)             -910              40
HF (g)               -270              170
SiF4 (g)            -1600             280
H2O (g)             -240              190

What is -72120 J/mol?

500

Suppose a first-order reaction has k = 37.5 s-1 and [A]o = 0.127 M. How long will it take for 75% of the reactant A to be consumed?

What is 0.037 s?

500

Determine the minimum pressure of N2 required to keep this a spontaneous reaction at 298 K. 

N2 + 3 H2 -> 2NH3 (all gas) delta G = -33.3 kJ/mol

PH2 = 0.01 atm

PNH3 = 1 atm

What is PN2 > 1.46 atm.


500

A 30.0 ml of solution of 0.200 M HOCl is titrated with a 0.400 M KOH soln (Ka HOCl = 4.0 x 10-8). Calc pH when 15.0 ml of NaOH was added.

What is 10.26 pH?

500

Calculate the Eq constant at T = 25 °C. 

Pb2+ (aq) + Sn(s) -> Sn2+(aq) + Pb(s)

What is k = 2.84 x 106