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

because of all the things that happen around the us, many people get into arguments which sadly could get physical, but we should actually make a change for that.