Use the problem below to answer the question: 34 grams of carbon reacted with an unlimited amount of H2O. The reaction is: C + H2O → CO + H2 The atomic mass of C is 12.01 g/mole. The atomic mass of H2 is 2.016 g/mole. Finish the problem by choosing the correct format for dimensional analysis.

There will be produced 79.30 grams of CO and 5.707 grams of H2

Explanation:

The complete question:

Work the entire problem from the beginning.

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

C + H2O → CO + H2

The atomic mass of C is 12.01 g/mole. The atomic mass of H2 is 2.016 g/mole.

Step 1: Data given

Mass of carbon = 34.00 grams

H2O is in excess

Molar mass of carbon = 12.01 g/mol

Molar mass of H2 = 2.016 g/mol

Step 2: The balanced equation

C + H2O → CO + H2

Step 3: Calculate moles of carbon

Moles carbon = Mass carbon / molar mass of carbon

Moles carbon = 34.00 g / 12.01 g/mol

Moles carbon = 2.831 moles

Since carbon is the limiting reactant. it will completely be consumed. There won't remain any carbon.

Step 4: Calculate moles of H2O

For 1 mol carbon we need 1 mol of H2O

For 2.831 mol of carbon we need 2.831 moles of H2O

Mass of H2O = 18.02 g/mol * 2.831 moles = 51.01 grams

There will react 51.01 grams of H2O

Step 5: Calculate moles of CO and H2

For 1 mol C we need 1 mol of H2O to produce 1 mol of CO and 1 mol of H2

For 2.831 mol of C and 2.831 mol of H2O we'll have 2.831 mol of CO and 2.831 mol of H2

Step 6: Calculate mass of CO and H2

Mass of CO = 2.831 moles * 28.01 g/mol = 79.30 grams

Mass of H2 = 2.831 moles * 2.016 g/mol = 5.707 grams

There will be produced 79.30 grams of CO and 5.707 grams of H2