Question

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

Answer 1

a) 0.67 moles of O2

b) 1.34 moles H2O

c) 24.15 grams of H2O

d) 21.44 grams O2

Step-by-step explanation:

Step 1: Data given

Dihydrogen dioxide = H2O2

oxygen gas = O2

Moles H2O2 = 1.34 moles

Molar mass of H2O2 = 34.01 g/mol

Step 2: The balanced equation

2H2O2 → 2H2O + O2

Step 3: Calculate moles of H2O formed

For 2 moles H2O2 we'll have 2 moles H2O produced

For 1.34 moles H2O2 we have 1.34 moles H2O produced

This is 1.34 moles * 18.02 g/mol = 24.15 grams of H2O

Step 4: Calculate moles of O2 formed

For 2 moles H2O2 we'll have 1 mol O2 produced

For 1.34 moles H2O2 we'll have 1.34 /2 = 0.67 moles of O2 produced

This is 0.67 moles * 32.00 g/mol = 21.44 grams O2

Answer 2

The answer to your question is

a) 0.67 moles of O₂

b) 1.34 moles of H₂O

c) 24.12 g of water

d) 10.72 g of O₂

Step-by-step explanation:

Chemical Reaction

2H₂O₂ (aq) ⇒ 2H₂O (l) + O₂ (g)

Data

1.34 moles of H₂O₂

To solve this problem use proportions

a)

2 moles of H₂O₂ ----------------- 1 mol of O₂

1.34 moles of H₂O₂ -------------- x

x = (1.34 x 1) / 2

x = 0.67 moles of O₂

b)

2 moles of H₂O₂ ------------------ 2 moles of H₂O

1.34 moles of H₂O₂ -------------- x

x = (1.34 x 2)/ 2

x = 1.34 moles of H₂O

c)

18 g of H₂O ------------------- 1 mol

x -------------------- 1.34 moles

x = (1.34 x 18) / 1

x= 24.12 g of water

d)

16 g of O₂ -------------------- 1 mol

x ------------------- 0.67 moles

x = (0.67 x 16) / 1

x = 10.72 g of O₂