H2 + Cl2 <----> 2 HCl. When some Cl2 is removed the equilibrium will shift in this direction and the Keq will undergo this change at constant temperature.
What is shift left and no change in Keq
100
These are three examples of strong acids other than HCl and HBr.
What are HI, H2SO4, HNO3, HClO3, HClO4.
100
The approximate equivalence point pH when aqueous HNO3 is titrated with aqueous KOH.
What is 7.
100
The oxidation number of oxygen in K2O2.
What is -1.
100
The sign (+ or -) for the entropy change for each process.
(a) Br2(g) --> 2Br(g)
(b) Ca(2+)(aq) + CO3(2-)(aq) --> CaCO3(s)
(c) a new deck of cards is shuffled
What are (a) +, (b) -, (c) +
200
N2 + 3 H2 <----> 2 NH3 delta H = (-); upon warming the equilibrium will shift in this direction and the value of Keq will change in this way.
What is shift left and Keq will decrease.
200
This is the definition of Lewis acid and the identity of the Lewis acid in the following equation:
Al3+ + 6H2O <---> Al(H2O)6^(3+)
What is an electron pair acceptor and Al3+.
200
The combination given here that could not act as a buffer:
HNO3/KNO3 CH3NH2/CH3NH3Cl Na2CO3/NaHCO3 NH4Cl/NH3 HF/NaF
What is HNO3/KNO3
200
The balanced equation for H2O2 + Ag --> Ag+ + H2O under acidic conditions.
What is 2H+ + H2O2 + 2 Ag --> 2 Ag+ + 2 H2O
200
The signs of delta S, delta G and delta H for the process in which ammonium chloride dissolves in water and the beaker feels cool as the solution forms.
What is delta H is +, delta G is (-), and delta S is (+).
300
The value of Q and the shift direction for the reaction,
PCl3(g) + Cl2(g) <---> PCl5(g) having Kc = 0.18 and [PCl3] = 0.0420, [Cl2]= 0.0240, and [PCl5] = 0.00500.
What is Q = 4.96 and the reaction will shift left.
300
The pH of a 0.0015 M Mg(OH)2 solution.
What is 11.48
300
The pH of a buffer consisting of 0.20 M HCN and 0.30 M KCN given that Ka HCN = 6.2 x 10^(-10)
What is 9.38.
300
The cell voltage and identity of the cathode metal in a Ni/Pb standard cell.
Ni(2+) + 2e --> Ni E = -.25 v
Pb(2+) + 2e --> Pb E = -.13 v
What is .12 v and Pb is the cathode.
300
The second law of thermodynamics.
What is the entropy of the universe increases with any spontaneous process.
400
This is the Kc for the equation: 2HBr(g) <----> H2(g) + Br2(g) if the equilibrium concentration of Br2 is 0.0955 M when 2.00 mole of HBr is initially put into a 4.00 L container.
What is 0.0225?
400
The pH of 0.25 M acetic acid having Ka = 1.8 x 10^(-5).
What is 2.67.
400
The Ksp of silver carbonate which has [CO3^(2-)] = 1.3 x 10(-4) in a saturated solution.
What is 8.8 x10(-12).
400
The moles of copper metal produced from CuSO4 solution during the eletroplating of a spoon with a current of 1.2 A for 5 minutes.
What is .0019 mole.
400
The enthalpy change for a reaction having delta G = -130 kJ/mole and delta S = 45 J/K at 50 C.
What is -115 kJ.
500
These are the equilibrium concentrations of each gas when 0.240 mole each of SO3 and NO are put in a 2.00 L container and allowed to reach equilibrium.
SO3(g) + NO(g) <---> NO2(g) + SO2(g) with Kc = .500
What are [SO3] = [NO] = .0497 and [NO2] = [SO2] = .0703
500
The pH of 0.10 M methylamine is 11.81. This is the Kb of methylamine.
What is 4.5 x 10^(-4).
500
The value of Q and expected observation of a precipitate or not when 100. mL of 1.0 x 10(-2) M KCl is mixed with 100. mL of 2.0 x 10(-2) M Pb(NO3)2.
Given Ksp PbCl2 = 1.7 x 10(-5)
What is Q = 2.5 x 10 (-7) so no ppt will form because Q < K.
500
The balanced half-reaction that occurs during the oxidation of water.
What is 2H2O --> O2 + 4H+ + 4e-
500
These Choate dorm names can be spelled using chemical element symbols. For example SOHO = sulfur(S)/oxygen(O)/hydrogen(H)/oxygen(O). No other names are abbreviations.
What are Pierce, Tenney House, Walsh, Atwater, ...?