When chromium metal is added to nitric acid, the following reaction takes place
Cr (s) + 6 HNO3 (aq) + Cr(NO3)3 (aq) + 3 H2O (1) + 3,
NO2 (g)
Calculate the volume of NO2 gas (in L) collected over
water at 40.0 °C when 11.1 g of chromium is added to
excess nitric acid if the total pressure is 675.0 torr. The
vapor pressure of water at 40.0 °C is 55.3 torr.

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:

no but i do not usually comment or use my voice that much when it comes to social media