Answer:
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
