
3/6 SI Session
Authored by Emily Ruz
Chemistry
University
Used 1+ times

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13 questions
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1.
OPEN ENDED QUESTION
1 min • 1 pt
What change would we expect to see once the reaction reaches equilibrium?
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2.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How do we know how quickly the reaction reaches equilibrium?
By watching it
By the rate law
By looking it up online
3.
OPEN ENDED QUESTION
5 mins • 1 pt
How do we write the forward and backward elementary reaction for the following reaction?
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Answer explanation
forward: R = k1[NO2]2
backward: R = k-1[N2O4]
at equilibrium:
k1[NO2]2 = k-1[N2O4]
k1/k-1 = [N2O4]/[NO2]2
4.
OPEN ENDED QUESTION
3 mins • 1 pt
Identify the variables of the equilibrium expression.
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Answer explanation
Kc molar equilibrium constant
[A], [B], [C], [D] concentrations of A, B, C, D
in mol/L
a, b, c, d
stoichiometric coefficients
5.
OPEN ENDED QUESTION
3 mins • 1 pt
Identify the variables of the equilibrium expression.
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Answer explanation
Kp molar equilibrium constant
PA, PB, PC, PD
partial pressures of A, B, C, D
in atm
a, b, c, d
stoichiometric coefficients
6.
MULTIPLE CHOICE QUESTION
30 sec • Ungraded
Can we use KP and Kc interchangeably?
Yes
No
Maybe?
Answer explanation
Yes!
KP = Kc(RT)^Δn
Δn = moles gas product - moles gas reactant
R = 0.082 atm L/mol K
T in kelvin
7.
OPEN ENDED QUESTION
3 mins • 1 pt
General rules for writing equilibrium constants:
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Answer explanation
1. do not include pure solids/liquids
2. do not include water when it is the solvent
3. Kc uses molarities, Kp uses partial pressures
4. Kc and Kp are dimensionless
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