When the following equation is balanced using the smallest whole number coefficients,

Cr₂(SO₄)₃ + RbOH --------> Cr(OH)₃ + Rb₂SO₄

the sum of all the coefficients is

When iron pyrite (FeS₂) is heated in air, the process known as "roasting" forms sulfur dioxide and iron(III) oxide. When the equation for this process is completed and balanced, using the smallest whole number coefficients, what is the coefficient for "O₂"?

___ FeS₂ + ___ O₂ ___ SO₂ + ___ Fe₂O₃

2H₂ + O₂ → 2H₂O

How many moles of water can be made from 100 g of hydrogen?

(RAM of H = 1, RAM of O = 16)

For the Balanced Reaction: 3Mg + Fe₂O₃ → 3MgO + 2Fe; What is the moles of iron produced when 2.4g magnesium react with excess iron (III) oxide ? (RAM Mg = 24, Fe = 56)

2Al + 3H₂SO₄ ---> Al₂(SO₄)₃ + 3H₂

How many grams of aluminum sulfate would be formed if 5.4g of aluminum completely reacted with sulfuric acid? (RAM Al = 27, RMM Al₂(SO₄)₃ = 342)

Fe + S → FeS

0.8 moles of Fe are allowed to react an excess of S. What is the mass of FeS produced?

(RAM of Fe = 56, RAM of S = 32)

2CO + O₂ → 2CO₂

What is the volume of CO₂ produced at room temperature when 16 g of O₂ with an excess of CO?

(RAM of C = 12, RAM of O = 16)

2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O

What is the mass of C₂H₆ used to produce 88g of CO₂?

(RAM of C = 12, RAM of H = 1, RAM of O = 16)

CH₄ + 2O₂ → CO₂ + 2H₂O

24 g of CH₄ will produce how many grams of water?

(RAM of C = 12, H = 1, O = 16)