A carboxylic acid obtained from the root of a tree is made up of carbon,

hydrogen and oxygen. Burning $1,000$ g of the acid yielded $2\mathrm{.}497$ g of carbon dioxide and $0\mathrm{.}6495$ g of water.

$2\mathrm{.}497$ g of carbon dioxide and $0\mathrm{.}6495$ g of water. Knowing that the molar mass of the acid is $388\mathrm{.}46$ g$,$ determine

the empirical and molecular formula of the compound.