2C4H10 + 13 02 - - 8 CO2 + 10H20

If i want to produce 50g of H20 using the above combustion reaction, how many mol of C4H10 should i use?

0.55 mol C4H10

10 mol C4H10

2.77 mol C4H10

3.79 mol C4H10

We should use 0.55 moles C4H10 to produce 50 grams of H2O (option 1 is correct)

Explanation:

Step 1: data given

Mass of H2O = 50 grams

Molar mass H2O = 18.02 g/mol

Molar mass C4H10 = 58.12 g/mol

Step 2: The balanced equation

2C4H10 + 13 02 → 8 CO2 + 10H20

Step 3: Calculate moles H2O

Moles H2O = 50.0 grams / 18.02 g/mol

Moles H2O = 2.77 moles

Step 4: Calculate moles C4H10

For 2 moles C4H10 we need 13 moles O2 to produce 8 moles CO2 and 10 moles H2O

For 2.77 moles H2O we need 2.77/5 = 0.55 moles C4H10

We should use 0.55 moles C4H10 to produce 50 grams of H2O (option 1 is correct)