Dihydrogen dioxide decomposes into water and oxygen gas. calculate the amounts requested if 1.34 moles of dihydrogen dioxide react according to the equation.
you must show all units.
a. moles of oxygen formed
b. moles of water formed
c. mass of water formed
d. mass of oxygen formed

Answers:

a. Moles of oxygen formed: 0.670 mol

b. Moles of water formed: 1.34 mol

c. Mass of water formed: 24.1 g

d. Mass of oxygen formed: 21.4 g

Explanation:

Dihdyrogen dioxide is the chemical name for a compound made of two hydrogen atoms and two oxide atoms, i.e. H₂O₂, which is also known as hydrogen peroxide or oxygenated water.

The decomposition reaction of dihydrogen dioxide into water and oxygen gas is represented by the balanced chemical equation:

The mole ratios derived from that balanced chemical equation are:

a. Moles of oxygen formed

When you solve for x, you get:

b. Moles of water formed

When you solve for x, you get:

c. Mass of water formed

Using the number of moles of water calculated in the part b., you calculate the mass of water formed, in grams, using the molar mass of water:

       ⇒ mass in grams = number of moles × molar mass

       ⇒ mass in grams = 1.34 mol × 18.015 g/mol = 24.1 g

d. Mass of oxygen formed

Using the number of moles of oxygen determined in the part a., you calculate the mass in grams using the molar mass of O₂.

the millers tale is the answer.

2b2t

explanation:

2b2t