Not a questionCan Someone Verify My Balancing Chemical Equations Homework?

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The user seeks verification for balancing chemical equations in preparation for a test, providing images of their work. Respondents note issues with the formatting of the images, suggesting they be resized for easier viewing. They question the choice of Li2O over LiOH and indicate that methane appears incorrect. Additionally, they highlight the need for the lowest possible integer coefficients in the equations and point out the non-existence of KSO4. Accurate balancing of chemical equations is crucial for success in chemistry assessments.
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Homework Statement



Could someone verify if these are correct, my text does not provide answers and i have a test tom.

Thank you very much.

http://img251.imageshack.us/img251/9319/lastscanx.jpg
http://img251.imageshack.us/img251/886/lastsc1an.jpg
http://img136.imageshack.us/img136/8292/lasts3can.jpg
 
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Bump please
 
Don't post pictures that wide, resize them to some reasonable size. Scrolling screen left and right to read what you have written is irritating. I have just skimmed.

Why Li2O and not LiOH? Is that product you were given?

Methane looks wrong.

BaSO4 precipitation - these should be lowest possible integeres, and no such substance as KSO4.

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Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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