What mass of carbon dioxide, water, and sulfur dioxide can be produced from the combustion of 1.5793g of C7H12S?

RMM of C7H12S = 128 (approx.)

Mass = 1.5793g

Mass of Carbon
= 1.5793*(84/128)
=1.036416 g
Mass of Carbon Dioxide
= 1.03642 g *(44/12)
= 3.80019 g
= 3.8002 g (to 5 significant figures)

Since the original mass is given to 5 significant figures, you will need to replace the relative atomic masses above with ones of similar accuracy.

The calculation of H2O and SO2 are similar.

the h20 and s02 you do not have any carbon though to work with it?

You would replace carbon with H and CO2 with H2O, similarly for S and SO2.

To find the mass of carbon dioxide (CO2), water (H2O), and sulfur dioxide (SO2) produced from the combustion of C7H12S, we need to balance the chemical equation representing the combustion reaction and use stoichiometry.

The balanced chemical equation for the combustion of C7H12S is:
C7H12S + 9O2 -> 7CO2 + 6H2O + SO2

Step 1: Calculate the molar mass of C7H12S.
The molar mass of carbon (C) is 12.01 g/mol, the molar mass of hydrogen (H) is 1.01 g/mol, and the molar mass of sulfur (S) is 32.06 g/mol.
So, the molar mass of C7H12S is:
7(12.01 g/mol) + 12(1.01 g/mol) + 32.06 g/mol = 100.23 g/mol

Step 2: Calculate the number of moles of C7H12S.
To do this, we use the formula:
moles = mass / molar mass
moles = 1.5793 g / 100.23 g/mol ≈ 0.0157 mol (rounded to four decimal places)

Step 3: Use stoichiometry to find moles of CO2, H2O, and SO2 produced.
From the balanced equation, we can see that 1 mole of C7H12S reacts to produce 7 moles of CO2, 6 moles of H2O, and 1 mole of SO2.
Therefore:
moles of CO2 = 7 × moles of C7H12S = 7 × 0.0157 mol = 0.1099 mol
moles of H2O = 6 × moles of C7H12S = 6 × 0.0157 mol = 0.0942 mol
moles of SO2 = 1 × moles of C7H12S = 1 × 0.0157 mol = 0.0157 mol

Step 4: Calculate the mass of CO2, H2O, and SO2.
To do this, we use the formula:
mass = moles × molar mass

Mass of CO2 = 0.1099 mol × (12.01 g/mol) ≈ 1.319 g (rounded to three decimal places)
Mass of H2O = 0.0942 mol × (18.02 g/mol) ≈ 1.695 g (rounded to three decimal places)
Mass of SO2 = 0.0157 mol × (64.06 g/mol) ≈ 1.004 g (rounded to three decimal places)

Therefore, approximately 1.319 grams of carbon dioxide, 1.695 grams of water, and 1.004 grams of sulfur dioxide can be produced from the combustion of 1.5793 grams of C7H12S.