If 23.7g of C8H18 are combusted, what mass of water will be produced?

To determine the mass of water produced when 23.7g of C8H18 is combusted, we need to use the balanced chemical equation for the combustion of C8H18:

C8H18 + 12.5O2 -> 8CO2 + 9H2O

From the balanced equation, we can see that for every 1 mole of C8H18 combusted, 9 moles of water are produced.

To find the moles of C8H18 present in 23.7g, we need to calculate the molar mass of C8H18:

(12.01 * 8) + (1.01 * 18) = 114.23 g/mol

Now we can calculate the moles of C8H18:

moles = mass / molar mass
moles = 23.7g / 114.23 g/mol ≈ 0.2077 moles

Since the mole ratio between C8H18 and water is 1:9, we can calculate the moles of water produced:

moles of water = moles of C8H18 * (9 moles of water / 1 mole of C8H18)
moles of water = 0.2077 moles * (9 moles of water / 1 mole of C8H18) ≈ 1.8693 moles

Finally, we can calculate the mass of water produced:

mass = moles * molar mass
mass = 1.8693 moles * (18.02 g/mol) ≈ 33.70g

Therefore, when 23.7g of C8H18 is combusted, approximately 33.70g of water will be produced.

To find the mass of water produced when 23.7g of C8H18 (octane) is combusted, we need to use the balanced chemical equation for the combustion reaction.

The balanced equation for the combustion of octane is:
C8H18 + 12.5O2 → 8CO2 + 9H2O

From the balanced equation, we can see that for every 1 mole of octane combusted, we produce 9 moles of water.

To determine the number of moles of octane present in 23.7g, we need to calculate the molar mass of octane (C8H18), which is:
(8 * atomic mass of carbon) + (18 * atomic mass of hydrogen)

Using the atomic masses from the periodic table:
Carbon (C): 12.01 g/mol
Hydrogen (H): 1.01 g/mol

Calculating the molar mass:
Molar mass of C8H18 = (8 * 12.01) + (18 * 1.01) = 114.23 g/mol

Now, we can calculate the number of moles of octane by dividing the given mass by the molar mass:
Moles of octane = Mass (g) / Molar mass (g/mol) = 23.7g / 114.23 g/mol

Next, we can use the mole ratio from the balanced equation to determine the number of moles of water produced. Since the mole ratio is 1:9 (1 mole of octane produces 9 moles of water), we multiply the moles of octane by the ratio:
Moles of water = Moles of octane * 9

Finally, we can calculate the mass of water produced by multiplying the number of moles of water by the molar mass of water (H2O), which is: 18.02 g/mol.
Mass of water = Moles of water * Molar mass of water

By following these steps, you can find the mass of water produced when 23.7g of C8H18 is combusted.

First establish the combustion equation and have it balanced:

C8H18 + O2 -> 8CO2 + 9H2O.
Balances for C, but not for O.
Since there are 16+9=25O on the right, we need to double the number to make the number of molecules on the left a whole number. So it becomes:
2C8H18 + 25O2 -> 16CO2 + 18H2O.

Next step is to observe the relative molecular masses in 8H18 and 18H2O.

You can then calculate the mass of H2O produced by proportions using 23.7g of octane.

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