The mass in grams, to five sig figs, of carbon dioxide produced when 22.031 grams of c6h6 is combusted is the same as the mass of the least common isotope of element x?

74.566

Explanation:

C6H6 + 02 =6CO2 + 3H2O

2C6H6 + 15O2=12CO2 + 6H2O

mm of C6H6=(12x6)+(6x1)= 72+6 =78gram/mol

mass conc = 2x78=156

mm CO2= 12+(16x2)=

12+32= 44gram/mol

mass conc of CO2 = 12x44

=  528

from The equation

156g of C6H6=528g of CO2

22.031g of C6H6=Xg of CO2

therefore, Xg=

22.031 x 528/ 156

= 74.566g

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: