The balanced chemical equation for the combustion of propane is C3H8(g)+5O2(g) --> 3CO2(g)+4H2O(g) Which statement is correct about the complete combustion of 3.00 mole of propane, C3H8? \rm C_3H_8(g) + 5 O_2(g) --> 3 CO_2(g) + 4 H_2O(g)Which statement is correct about the complete combustion of 3.00 mole of propane, \rm C_3H_8?1. 12.00 mol H2O are produced.2. 3.00 g CO2 are produced.3. 3.00 mol CO2 are produced.4. 12.00 g H2O are produced

The correct statement about the complete combustion is 12 moles

Explanation:

We are given:

Moles of propane = 3.00 moles

To calculate the number of moles, we use the equation:

    ......(1)

For the given chemical equation:

By Stoichiometry of the reaction:

1 mole of propane produces 3 moles of carbon dioxide

So, 3.00 moles of propane will produce = of carbon dioxide

Now, calculating the mass of carbon dioxide from equation 1, we get:

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 9 moles

Putting values in equation 1, we get:

By Stoichiometry of the reaction:

1 mole of propane produces 4 moles of water

So, 3.00 moles of propane will produce = of water

Now, calculating the mass of water from equation 1, we get:

Molar mass of water = 18 g/mol

Moles of water = 12 moles

Putting values in equation 1, we get:

Hence, the correct statement about the complete combustion is 12 moles

explanation:

i think option no d is the correct answer