I finished the problem like this:
(10.52g NO2)(1 mole NO2/46.01g NO2)(4 moles HNO2/4 moles NO2)(47.02g HNO2/1 mole HNO2)=10.75g HNO2
10.75g HNO2 x .6=6.45g Acid rain produced.
Looks OK to me, although I have just skimmed the calculations.
And with the N+O instead of N2+O2, are you sure that would not change the result? I would think that it would because the formula mass would be different in my first step of the problem. Am i right or is it alright leaving it how it is?
Changing to N
2 and so on will not change calculation result, as it doesn't change molar ratio - there is 1 molecule produced per every atom of nitrogen. But you better change to your reaction to N
2 version, as we always put diatomics as such into equations.
Also, I still do not have any idea to approach the first problem. Thanks for all of your help
As for the first problem - I would start with the balanced reaciton equation of glucose oxidation. But then I have no idea what it means by "respiring glucose". Either it is some error in the text or my English fails me. I can guess that it is really about glucose oxidation and that this oxidation is not complete, so that there is only 15% of expected CO
2 produced - but even then, this information is irrelevant to the question, as all you can do is to find mass of glucose that reacts with given amount of oxygen.
Perhaps someone else will have an idea what is going on, question doesn't make sense to me.