Methylhydrazine, ch6n2, is commonly used as a liquid rocket fuel. the heat of combustion of methylhydrazine is −1.30 × 103 kj/mol. how much heat is released when 206.2 g of methylhydrazine is burned? if appropriate, express your answer in scientific notion. (click on the answer box to show the pallet.)

Explanation:

Given that:

The heat of combustion of methylhydrazine =

It means that:

1 mole of methylhydrazine on combustion, releases of energy

Molar mass of ‎methylhydrazine = 46.072 g/mol

Means that, 1 mole of methylhydrazine contains 46.072 g of methylhydrazine

Thus,

46.072 g of methylhydrazine on combustion, releases of energy

Also,

1 g of methylhydrazine on combustion, releases of energy

206.2 g of methylhydrazine on combustion, releases of energy

Heat released =

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: