When an unknown amount of methane reacts with 40.7 g of chlorine, 40.5 g of methyl chloride and 36.5 g of hydrogen chloride form how much methane was used round to the tenth

36.3 gram

Explanation:

CH₄ + Cl₂ = CH₃Cl + HCl

In any reaction , mass is conserved

mass of product = 40.5 + 36.5 = 77 g

Let methane reacted be x .

mass of reactant = x + 40.7

mass of reactant = mass of product

x + 40.7  = 77

x = 36.3 gram

methane reacted = 36.3 gram.

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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: