Unit 9
Unit 8
Unit 7
Unit 6
Unit 5
100
This combination of enthalpy and entropy drives a reaction that is thermodynamically favorable at all temperatures.
What is -H, +S (resulting in G < 0)?
100
By calculating pH, you are describing the concentration of this ion.
What is [H+]?
100
The equilibrium expression of the formation of ammonia, N2 + 3H2 -> 2NH3
100
The name of this laboratory set up. 
What is a calorimeter?
100
Three ways to speed up a chemical reaction.
What is 1) add a catalyst, 2) increase surface area, 3) increase reactant concentration, 4) increase temperature, 5) agitation?
200
The half-cell the anions of the salt bridge flow towards.
What is the anode?
200
The ion concentration represented by "x" in a weak acid equilibria RICE table.
What is the [H+] for a weak acid?
200
This phase is not included in the equilibrium expression.
What is solid?
200
The amount of energy required to raise the temperature of one gram of a substance by one degree Celsius.
What is specific heat capacity?
200
The rate law for an elementary step of 2A + B → C + D
What is Rate = k [A]2[B] ?
300
The cell voltage change when the Q > K.
What is decrease?
300
The pH of a salt containing conjugates of strong acid/base (ex. NaBr).
What is neutral?
300
The manipulation of K when a reaction is reversed.
What is 1/K?
300
The enthalpy of the following reaction:
What is -186 kJ/mol?
300
The order of a reaction when the concentration doubles and the initial rate quadruples.
What is second order?
400
The half-cell that gains mass in a galvanic electrochemical cell.
What is the cathode?
400
The pH at the midpoint of a titration of a weak acid with a strong base.
What is pH = pKa?
400
The two things that do not shift an equilibrium.
What are catalysts and inert gases?
400
The heat absorbed by 2.76 kg of a substance with a specific heat capacity of 0.562 J/g*C) is heated from 20.5oC to 24.5oC.
What is 6.20 x 103 J?
400
The step of the reaction mechanism that determines the rate law.
What is the slow step?
500
This phenomenon is observed when the decomposition of hydrogen peroxide H2O2 -> H2O + O2, which is a spontaneous reaction, does not occur at room temperature.
What is kinetic control?
500
The pH when 100 mL of 0.10 M HC2H3O2 is titrated with 50 mL of 0.10 M NaOH. (The Ka of HC2H3O2 = 1.8 x 10-5)
What is 4.75?
500
This reaction occurs in a container with a moveable piston. This is the shift in equilibrium when the volume of the container is decreased.
What is toward the products/forward?
500
What is +318.85 kJ?
500
The reaction order that has a consistent half-life.
What is 1st order?