The balanced chemical equation for the combustion of propane is

C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)
C3 H 8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

Which statement is correct about the complete combustion of 3.00 mole of propane, C3H8?

a. 12.00 mol H2O are produced.
b. 3.00 g CO2 are produced.
c. 3.00 mol CO2 are produced.
d. 12.00 g H2O are produced.

Option a. 12.00 mol H2O are produced.

Explanation:

C3H8 + 5O2 → 3CO2 + 4H2O

From equation,

1mole of C3H8 produce 4moles of H2O.

Therefore, 3moles of C3H8 will produce = 3 x 4 = 12moles of H2O

Option A is correct 12.00 mol H2O are produced.

Explanation:

Step 1: Data given

Number of moles of propane = 3.00 moles

Step 2: The balanced equation

C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)

Step 3: Calculate moles

For 1 mol propane we need 5 moles O2 to produce 3 moles of CO2 and 4 moles H2O

For 3.00 moles propane we need:

5*3.00 = 15.00 moles O2

3*3.00 = 9.00 moles CO2

4*3.00 = 12.00 moles H2O

Step 4: Calculate mass

Mass = moles * molar mass

Mass H2O = 12.00 mol * 18.02 g/mol

Mass H2O = 216.2 grams

Mass CO2 = 9.00 moles * 44.01 g/mol

Mass CO2 = 396.1 grams

Option A is correct 12.00 mol H2O are produced.

2b2t

explanation:

2b2t

1 is the answer to this problem