How many molecules of so2 are in 2.45 g of so2? (molar mass=64.06 g/mol). (hint: you need to use your entire stoichiometry flow chart! ) 0.0382 molecules 9.45 x10^25 molecules 2.30 x 10^22 molecules 6.35 x 10^-26 molecules

Answer is: 2.30 x 10^22 molecules.
m(SO₂) = 2,45 g- mass of sulfur(IV)-oxide.
M(SO₂) = 64,06 g/mol- molar mass of sulfur(IV)-oxide.
n(SO₂) = m/M = 2,45g ÷ 64,06 g/mol = 0,038 mol - amount of substance
N(SO₂) = n·Na = 0,038 mol · 6,022·10²³ 1/mol = 2,3·10²².
Na- Avogadro number(constant)- 6,022·10²³ 1/mol

Answer: abeexplanation:

1. the question asks the most appropriate, which seems to rule out "all of the above." your choice appears to be the correct one.

2. the protocol described is good for identifying correlation, but not cause and effect. for cause/effect, you need to devise a protocol that will assign the treatment (or not) to groups that have essentially the same "demographics" with respect to all the other variables. your choice regarding control group seems appropriate. random assignment of treatment (choice d) may be appropriate also. (i think you can argue that b and d are just different descriptions of the same method.)

3. d will randomize the birds, but may not guarantee there are 10 in each group. e will do both, so seems the better choice.

comment on question 2

based on the problem statement, it seems clear that confident, attentive drivers are more likely to use daytime running lights. so, the protocol might need to be devised in such a way that the lights would be turned on or off without the driver's knowledge. (an attentive driver will figure it out.) assigning a confident, attentive driver to a group required to drive without running lights might mess with his/her confidence and attentiveness. you don't want your experiment to do that. (nor do you want the experiment to subject a driver to greater risk of accident as a consequence of driving without running lights.) experiments involving human safety are always problematic.

7is b8 is d9 is c10 is a11 is d