Bonds
Heat / Equilibrium
Misc.
Calculations
Equations
100
What is the strongest kind of IMF
Hydrogen Bonds
100
Is this reaction endo or exo?
Endothermic, absorbs heat.
100
What is a polar molecule?
A molecule that has a charge on one side of the atom.
100
How do you calculate the number of moles?
Given weight/ molar mass of substance
100
What is avagadros number?
6.022 x 1023
200
Does Oxygen or Sulfur have a higher bond energy?
Sulfur, larger atom size which creates a stronger bond with its electrons.
200
Is melting ice endo or exothermic
Endo, ice absorbs heat from the surroundings to change states.
200
Draw the lewis structure for N2H4
(cant insert pic)
2 h bonded to each N, N-N bond, 2 lone electrons on each N atom
200
Find the number of moles in a 900ml 8M substance.
7.2 mol
200
what is charles law
v1/t2=v2/t2
300
Based on the octet rule, magnesium most likely forms what kind of ion?
Mg2+
300
increasing the volume shifts the reaction which direction?
Left, to favor the reactants
300
Does the slow or fast step determine the rate law?
The slow step, reaction can't happen any faster than this step.
300
What is the reverse rate constant if K1 is 7 x 10-12?
1 x 10-11
1/k1
300
Write the balanced net ionic equation for KOH + Fe(NO₃)₃ → KNO₃ + Fe(OH)₃
3OH⁻ (aq) + Fe⁺³ (aq) → Fe(OH)₃ (s)
400
How many equivalent resonance forms can be drawn for SO2 without expanding octet on the sulfur atom (sulfur is the central atom)?
3 structures
400
3 C2H2(g) → C6H6(g)
What is the standard enthalphy change ΔHo, for the reaction represented above?
(ΔHof of C2H2(g) is 230 kJ mol-1;
(ΔHof of C6H6(g) is 83 kJ mol-1;)
-607 Kj
400
What effect does a catalyst have on an equilibrium reaction?
Nothing. It has the same effect on both the backwards and forwards reaction.
400
What is the total mass of products formed when 16 grams of CH4 is burned with excess oxygen?
80 grams
400
What is the integrated rate law, straight line plot, and units for a 2nd order reaction?
(1/[A])= kt + (1/[Ao ])
1/A vs. T
L/mol x sec
500
The reaction below is used to produce methanol:
CO (g) + 2 H2 (g) ¬ CH3OH (l) DHrxn = -128 kJ
Calculate the C-H bond energy given the following data:
Bond D (kJ/mol)
C∏O 1072
HπH 436
CπO 358
OπH 463
1944 Kj
500
What is thermodynamically favorable?
Negative entropy, a negative enthalpy, and a negative Gibbs free energy value
500
Name 3 important solubility rules.
Compounds of NH4+ and group 1A metal ions are soluble.
Compounds of NO3–, ClO4–, ClO3– and C2H3O2– are soluble.
Compounds of Cl –, Br – and I – are soluble except those of Ag+, Cu+, Tl+, Hg22+ and Pb2+.
500
When 0.0322 mol of NO and 1.70 g of bromine are placed in a 1.00 L reaction vessel and sealed, the mixture reacts and the following equilibrium is established:
2NO(g) + Br2(g) ⇌ 2NOBr(g)
At 25.0 °C the equilibrium of nitrosyl bromide is 0.438 atm. What is the Kp?
Kp = 38.2
500
Write the Ksp expression for Zn3(AsO4)2(s) ⇌ 3Zn2+(aq) + 2AsO43¯(aq)
Ksp = [Zn2+]3 [AsO43¯]2