Monday, October 02, 2006
Monday Recap
G and D Honors:
We reviewed Dalton's Laws of Constant Composition and Multiple Proportions; I will dig up some worksheets on these laws and post them by tomorrow.
We then discussed the basis of the atomic mass scale. Don't freak out about that; practically speaking, you will be responsible for knowing simple conversions and ratios: for example, if one atom of Carbon "on average" weighs, 12.011 a.m.u., then a "mole" of Carbon atoms must weigh 12.011 grams....just replace the unit "a.m.u" with "grams" when you increase from one atom to one mole of atoms. The end.
Regents E: We reviewed Dalton's 4 Postulates on Atoms and then we did several examples of Dalton's Law of Constant/Definition Composition. We deduced whether two samples containing compounds of carbon and oxygen are actually samples of the same compound; we did this by applying the Law of Constant Composition.
AP: We finished some gas stoichiometry and then applied Dalton's Law of partial pressures to calculate the pressures of each component of a mixture of gaseous products. We then started another problem in which we will use the exact same law of partial pressures on a problem involving a mixture of gases collected over water (therefore, water vapor is always one of the gases in the mixture contributing to the total gas pressure of the mixture).
Tomorrow, we will hit that descriptive chem problem set and then cover one more gas law: Graham's Law of Effusion (done and done in Honors) and the Van der Waal's Gas Equation (child's play).
We reviewed Dalton's Laws of Constant Composition and Multiple Proportions; I will dig up some worksheets on these laws and post them by tomorrow.
We then discussed the basis of the atomic mass scale. Don't freak out about that; practically speaking, you will be responsible for knowing simple conversions and ratios: for example, if one atom of Carbon "on average" weighs, 12.011 a.m.u., then a "mole" of Carbon atoms must weigh 12.011 grams....just replace the unit "a.m.u" with "grams" when you increase from one atom to one mole of atoms. The end.
Regents E: We reviewed Dalton's 4 Postulates on Atoms and then we did several examples of Dalton's Law of Constant/Definition Composition. We deduced whether two samples containing compounds of carbon and oxygen are actually samples of the same compound; we did this by applying the Law of Constant Composition.
AP: We finished some gas stoichiometry and then applied Dalton's Law of partial pressures to calculate the pressures of each component of a mixture of gaseous products. We then started another problem in which we will use the exact same law of partial pressures on a problem involving a mixture of gases collected over water (therefore, water vapor is always one of the gases in the mixture contributing to the total gas pressure of the mixture).
Tomorrow, we will hit that descriptive chem problem set and then cover one more gas law: Graham's Law of Effusion (done and done in Honors) and the Van der Waal's Gas Equation (child's play).
# posted by C @ 4:35 PM 
