The alkenes are compounds of carbon and hydrogen with the general formula cnh2n. if 0.561 gram of any alkene is burned in excess oxygen, what number of moles of h2o is formed?

To solve this problem, we must first examine the chemical formula of an alkene (CnH2n) and notice that there are 2 H atoms for every 1 C atom. 

Therefore this means that we can calculate the weight percent of Hydrogen (H) using the molecular formula: 

wt% H2 = 2n * (1.0g/mol H)/[2n*(1.0g/mol H) + n*(12.0g/mol C)) x 100 = 14.3 wt% H

So for any alkene with mass of 0.561g, this contains (0.143)x(0.561g) = 0.080 g H 

Now, we calculate the number of moles of H this is by dividing with the molar mass: 

moles H = (0.080g H) / (1.00 g/mol H) = 0.08 moles H. 

We know that there are 0.5 moles of water per mole of hydrogen, therefore the moles of H2O formed is: 

moles H2O = 0.5 * moles H = 0.5 * (0.08) = 0.04 moles H2O

0.04 moles water

what are the statements?

explanation:

give me the statements and i'll tell you which is correct

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.