Your organization purchases bottles of a popular commercial solvent for resale. each bottle is labeled as containing 25.25 ounces of the solvent. your contract specifies that each bottle must contain 25.25 ± 0.1 ounces of the specified solvent. recently, you have noticed that some bottles appear to be out of specification. obviously, the most significant problem is bottles do not contain at least 25.15 ounces of solvent. the results of a study of the bottle-filling process indicate an average of 25.265 ounces of solvent in each bottle with a standard deviation of approximately 0.075 ounces. based on this information, what proportion of filled bottles are problematic? what is the total proportion out of tolerance?

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: