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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

Respuesta :

Answer: 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:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]     ......(1)

For the given chemical equation:

[tex]C_3H_8(g)+5O_2(g)\rightarrow 3CO_2(g)+4H_2O(g)[/tex]

  • For carbon dioxide:

By Stoichiometry of the reaction:

1 mole of propane produces 3 moles of carbon dioxide

So, 3.00 moles of propane will produce = [tex]\frac{3}{1}\times 3=9mol[/tex] 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:

[tex]9mol=\frac{\text{Mass of carbon dioxide}}{44g/mol}\\\\\text{Mass of carbon dioxide}=(9mol\times 44g/mol)=396g[/tex]

  • For water:

By Stoichiometry of the reaction:

1 mole of propane produces 4 moles of water

So, 3.00 moles of propane will produce = [tex]\frac{4}{1}\times 3=12mol[/tex] 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:

[tex]12mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(12mol\times 18g/mol)=216g[/tex]

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

12.00 moles H₂O will be produced. The correct statement is 1. 12.00 mol H2O are produced

Stoichiometry & Combustion

From the question, we are to determine which of the statements is correct

The given balanced chemical equation for the reaction is

C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g)

This means the complete combustion of 1 mole of propane (C₃H₈) needs 5 moles of oxygen (O₂), and it gives 3 moles of carbon dioxide (CO₂) and 4 moles of water (H₂O)

Now,

If 1 mole of propane on complete combustion gives 4 moles of water

Then,

3.00 moles of propane on complete combustion will produce 12.00 moles of water (H₂O)

Hence, 12.00 moles H₂O will be produced. The correct statement is 1. 12.00 mol H2O are produced

Learn more on Stoichiometry & Combustion here: https://brainly.com/question/14271082

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