Term
| When given standard reduction potentials, how can we tell which one is being oxidized and which one is being reduced? |
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Definition
| The one with the smaller potential is the one being oxidized |
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Term
What is the equation for E° Cell?
How do we tell what is being oxidized vs reduced? |
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Definition
E° Cell=E°reduced - E°oxidized
The one with the higher potential is reduced and the one with the lower is being oxidized |
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Term
| When given the E°cell how do we determine spontaneous vs non spontaneous reactions? |
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Definition
If the E°cell is positive it indicates a spontaneous reaction
If the E°cell is negative it indicates a non spontaneous reaction |
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Term
If we are told a reaction occurs in pure water what does that mean for Ka and Kb ? |
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Definition
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Term
What is the equation for Kw? |
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Definition
Kw= Ka * Kb
or
Kw= [ H3O+] * [OH-] |
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Term
When a reaction is under standard temperature and pressure what are the values for temperature ( in C and K) and pressure (atms)?
Also what does it mean for 1 mole of gas? |
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Definition
Temperature is 0ºC which is 273K
Pressure is 1 atm
1 mole of gas occupies a volume of 22.4 L
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Term
Graham's Law of Effusion tells us the relationship between rates of effusion and molar mass. Their relationship can be represented by? |
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Definition
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Term
The second law of thermodynamics states that for any spontaneous process the entropy of _________must _______ |
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Definition
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Term
Which type of radioactive decays causes a change in mass number? |
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Definition
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Term
The two types of radioactive decay that result in the same changes to mass and atomic numbers?
a. Gamma and Beta
b.Gamma and Positron emission
c. Positron emission and electron capture
d.Beta and electron capture
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Definition
C. Positron emission and electron capture
They both result in decrease in atomic number by one and an unchanged atomic mass
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Term
Deposition has what effect on ΔH and ΔS? |
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Definition
Deposition is turing a gas to a solid
This requires a loss of heat to the surroundings making
ΔH <0
Since we are making the molecules more ordered than they were
ΔS <0 |
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Term
| Enthalpy change for reactions where bonds are broken and formed what formula? |
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Definition
ΔH°reaction= ∑ ΔHbonds broken (reactants) - ∑ ΔHbonds formed (products)
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Term
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Definition
moles of solute over kg of solvent
(it is likely they will give a mass in grams and the amount of solvent in grams, we have to remember the equation and
use the molar mass to calculate moles of solute and rearrange to solve for kg of solvent) |
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Term
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Definition
| l Experimental - Theoretical l / Theoretical *100 |
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Term
| What is the mnemonic to help remember the solubility rules? |
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Definition
Soluble= NAG SAG
N for nitrates
A for acetate
G for group 1 ions
S for sulfates
A for ammonium
G for Group 17 halides
Insoluble= PMS
P= lead (Pb)
M= Mercury
S= Silver |
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Term
What is the difference between Paramagnetic and Diamagnetic? |
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Definition
Paramagnetic is known for having unpaired electrons
Diamagnetic is known for having paired electrons |
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