Question

Suppose you weigh the unknown substance on an electronic balance and find it has a mass of 445 grams. Analyzing the products of decomposition, you find that the masses of the elements in the sample are 232 grams of carbon, 58 grams of hydrogen, and 155 grams of oxygen. Finally, through further experimentation, you determine that the molar mass of the compound is 46.07 grams/mole.

Calculate the amount, in moles, of each component element in your substance. Use the periodic table to help you find the necessary molar masses.

____ moles of carbon

____ moles of hydrogen

____ moles of oxygen

Answer 1

To calculate the amount of moles of each element, divide the mass of each element by its molar mass. The substance contains 19.32 moles of carbon, 57.43 moles of hydrogen, and 9.69 moles of oxygen.

Step-by-step explanation:

To calculate the amount of moles of each component element in the substance, we need to use the given masses of the elements and the molar mass of the compound. First, calculate the mass of oxygen by subtracting the masses of carbon and hydrogen from the original mass of the substance:

Mass of oxygen = Mass of substance - Mass of carbon - Mass of hydrogen
Mass of oxygen = 445 g - 232 g - 58 g
Mass of oxygen = 155 g

Next, calculate the moles of each element by dividing their mass by their molar mass:

Moles of carbon = Mass of carbon / Molar mass of carbon
Moles of carbon = 232 g / 12.01 g/mol
Moles of carbon = 19.32 mol

Moles of hydrogen = Mass of hydrogen / Molar mass of hydrogen
Moles of hydrogen = 58 g / 1.01 g/mol
Moles of hydrogen = 57.43 mol

Moles of oxygen = Mass of oxygen / Molar mass of oxygen
Moles of oxygen = 155 g / 16.00 g/mol
Moles of oxygen = 9.69 mol

Answer 2

19.32 = moles of carbon

57.54 = moles of hydrogen

9.69 = moles of oxygen

Step-by-step explanation:

232 g carbon × 1 mol C / 12.011 g C= 19.32 mol C

58 g hydrogen × 1 mol H / 1.008 g H = 57.54 mol H

155 g oxygen × 1 mol O / 15.999 g O = 9.69 mol O