Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
5 Cards in this Set
- Front
- Back
|
Why does N2 have a lower boiling point than O2?
|
Nitrogen has a lower boiling point b/c less energy is required to overcome the van der Waals forces between the smaller N2 molecules (MM 28 vs. MM 32)
|
|
|
How to determine the number of moles present
|
divide the mass by the molar mass
e.g. # of moles of K present in 20g sample nK = mK/ MW K =(20g)/ (39.1 g/mol) = ~0.5 moles |
|
|
Enthalpy, (H)
Entropy,(S) Gibbs Free Energy (G) |
Enthalpy = (ΔH <0) exothermic
reaction; Spontaneous Entropy (S) = (ΔS > 0), Disorder Increases; Spontaneous Gibbs Free Energy= ΔG = ΔH – TΔS, Spontaneous if negative |
|
|
Determine Partial Pressure of H20 in rxn:
CH4 + O2 → CO2 + H2O total pressure = 1.2 torr |
CH4 + 2O2 → CO2 + 2H2O
PH2O = Ptotal × XH2O PH2O = 1.2 torr × 2/3 PH2O = 2.4 torr/3 PH2O = 0.8 torr |
|
|
Calculate the concentration of protons in solution with pH = 6.0
|
pH = –log[H3O+]
[H3O+] = 10^–pH [H3O+] = 10^–6 |
