In a 1.143e+2 g sample of iron(iii) oxide, how many grams of iron are present? your answer should have the appropriate number of significant figures (use two decimal places in atomic masses).

Mass of iron(III)oxide, Fe2O3 sample = 1.143*10^2 g

Molar mass of Fe2O3 = 159.69 g/mole

i.e. 1 mole of Fe2O3 weighs 159.69 g

Based on stoichiometry:

1 mole of Fe2O3 has 2 moles of Fe

Atomic mass of Fe = 55.85 g/mole

Therefore we can write:

159.69 g of Fe2O3 is composed of 2*55.85 g of Fe

Thus, amount of Fe present in 1.143*10^2 g sample of Fe2O3 is

= 1.143*10^2 * 2* 55.85/159.69

= 7.995*10^-1 g

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.