Liquid butane, C4H10, is stored in cylinders to be used
as a fuel. Suppose 35.5 g of butane gas is removed from a
cylinder. How much heat must be provided to vaporize this
much gas? The heat of vaporization of butane is 21.3 kJ/mol.

Explanation:

The heat to vaporize a liquid is equal to the amount of liquid in moles multiplied by the specific heat of vaporiztion per mole.

First, calculate the number of moles in 35.5g of butane.

Now, calculate the heat to vaporize that amount of liquid butane:

The answer must be reported with 3 significant figures.

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.