One method for the manufacture of "synthetic gas" is the catalytic reforming of methane with steam at high temperature and atmospheric pressure:
ch4 (g)+ h2o(g)→ co(g)+ 3h2 (g)
the only other reaction to be considered is the water-gas-shift reaction:
co (g)+ h2o(g)→ co2 (g)+ h2 (g)
if the reactants (methane and steam) are supplied in the ratio 2 mol steam to 1 mol methane, and if heat is supplied to the reactor so that the products reach a temperature of 1,300 k, the methane is completely converted and the product stream contains 17.4 mol% co.
1. assuming the reactants to be preheated to 600 k, calculate the heat requirement for the reactor?

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:

the role of the microscope world in creating new materials .

the answer is the first option

explanation:

just googled it m8. not that hard

lol