IMFs
Reaction Rates
Thermo&Equil
Acids & Bases
Electrochemistry
100

IMFs between molecules of liquid nitrogen N2 

What are London forces?

100

Rate at time zero of the reaction

What is an initial rate?

100

This thermodynamic function combines both enthalpy and entropy effects.

What is Gibbs Free Energy?

100

The conjugate acid corresponding to HPO42-

What is H2PO4-

100

The electrode where oxidation takes place

What is the anode?

200

IMFs found between any polar molecules

What are dipole-dipole forces?

200

In the equation: Rate=k[A]m [B]n    k is ______  and  m and n are called ___________

What are the rate constant and the orders with respect to A and B?

200

The following has the highest entropy at a given temperature: CO2(s), CO2(l) or CO2(g)

What is CO2(g)? 

200

The strongest acid in this series: HClO, HClO2, HClO3, HClO4

What is HClO4?

200

It will oxidize Chromium but not Nickel

What is Fe2+?

300

The molecule with the highest boiling point: Ethane (C2H6), Dichloromethane (CH2Cl2) or Butanol (CH3CH2CH2CH2OH)

What is butanol?

300

If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A.

What is second order?

300

If an endothermic reaction has a negative entropy, is this reaction spontaneous?

Non-spontaneous at all temperatures

300

Which of the following salts forms a basic solution when dissolved in water?

NH4Cl, NaClO4, KCl, CH3COONa

What is CH3COONa?

300

Which of these combinations would result in reaction? 

Al3+(aq) and Cu(s)

Cr2O72–(aq) and MnO4(aq)

Pb(s) and MnO4(aq)


What is Pb(s) and MnO4–(aq)?

400

All IMFs between acetone (CH3COCH3) and water 

What are London forces, dipole-dipole forces and hydrogen bonds?

400

Three factors that affect the rate of a reaction?

What are temperature, physical state of reactants and catalyst?

400

Predict the change in entropy for the following reaction:

2 H2S(g)  + 3 O2(g)  →2 SO2(g)  + 2 H2O(g)


Decreases (deltaS<0)

400

The pH of a 0.0200 M NaOH solution.

What is 12.3?

400

The standard cell potential (E°cell) of the reaction below is -0.34 V. Calculate the value of ΔG° for the reaction in kJ/mol.

Cu (s)  +  2H+ (aq)  →  Cu2+ (aq)  +  H2 (g)

What is 66 kJ/mol?

500

The following molecules are NOT miscible with water: propanol (CH3CH2CH2OH), hexane (C6H14), benzene (C6H6), octanol (C8H17OH)

What are hexane and benzene?

500

Sucrose decomposes in a first order process. If the half-life of sucrose is 3.21 h, what time is required for 75% of sucrose to decompose?

What is 6.42 h?

500

The Gibbs Free Energy for the dissolution of PbBr2 at 25.0 °C is + 32.4 kJ/mol .

PbBr2(s) ⇌ Pb2+(aq) + 2 Br-(aq)

Calculate the equilibrium constant, Keq, for the dissolution of PbBr2 at this temperature

2.09 x 10 -6

500

20.0 mL of 0.100 M HCl solution is titrated with 0.200 M NaOH solution at 25°C. Calculate the volume of NaOH solution (in mL) needed to reach the equivalence point.

What is 10 mL NaOH?

500

Calculate the voltage and the Gibbs free energy for a voltaic cell based on the reaction 

Fe2+ + Mg = Fe + Mg2+

What is 1.93 V and =-372 kJ?

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