How many grams of H2 would be formed if 34 grams of carbon reacted with an unlimited amount of H2O? The reaction is:

C + H2O CO + H2

1) Is this equation balanced?

2) What is the starting substance?

3) What is the ending substance that is asked for in the problem?

There is 5.72 grams of H2 formed

1) C + H2O → CO + H2

2) We start with 34 grams of carbon that will react with an excess of H2O

3) 5.72 grams of H2

Explanation:

Step 1: Data given

Mass of carbon = 34.00 grams

H2O is in excess

Molar mass of C = 12 g/mol

Molar mass of H2O = 18.02 g/mol

Step 2: The balanced equation

C + H2O → CO + H2

Step 3: What is the starting substance

We start with 34 grams of carbon that will react with an excess of H2O

Step 4: Calculate moles carbon

Moles C = mass C / molar mass C

Moles C = 34.00 grams / 12.00 g/mol

Moles C = 2.833 moles

Step 5: Calculate moles H2

Carbon is the limiting reactant.

For 1 mol Carbon we need 1 mol H20 to produce 1 mol CO and 1 mol H2

For 2.833 moles C we'll have 2.833 moles H2

Step 6: Calculate mass of H2

Mass H2 = moles H2 * molar mass H2

Mass H2 = 2.833 moles * 2.02 g/mol

Mass H2 = 5.72 grams of H2