A container is filled with 4.0 g and 5.0 g 02. The mixture is ignited produced water how much water is produced

The chemical reaction would be written as:

2H2 + O2 = 2H2O

We are given the amounts of the reactants thus we need to determine the limiting reactant before determining how much product is produced.

4.0 g H2 ( 1 mol / 2.02 g ) = 1.98 mol H2
5.0 g O2 ( 1 mol / 32 g ) = 0.1563 mol O2

The limiting reactant would be O2 since it would be consumed completely in the reaction.

0.1563 mol O2 ( 2 mol H2O / 1 mol O2 ) ( 18.02 g / mol ) = 5.6 g H2O is produced

vintechnology vintechnology · Answer 2 · 2022-03-17T09:34:56-04:00

The mass of water produced is 5.6 g

The reaction is between hydrogen gas and oxygen molecules. Therefore,

Chemical reaction:

H₂ + O₂ → H₂O

Let's balance the reaction before calculating the mass of water produced.

2H₂ + O₂ → 2H₂O

The limiting reagent is oxygen and it will determine the amount of product formed. Therefore,

32 g of oxygen = 36 g of water

5 g of oxygen = ?

cross multiply

mass of water formed = 36 × 5 / 32

mass of water formed = 180 / 32

mass of water formed = 5.625 g

mass of water formed = 5.6 g

learn more on chemical reaction here: https://brainly.com/question/15201964