Combustion analysis of 1.00g of the male sex hormone, testosterone, yields 2.90 g of CO2 and .875 g H2O. What are the mass percents of carbon, hydrogen, and oxygen in testosterone?
How do I solve this?
How many grams of C is in 2.90g of CO2? That is the same mass of C in the 1 gram of testerone.
How many grams of H are in .875 g of water? That is the same mass of H in the 1 gram of testerone.
Now, to figure the O in testostrone, subtract the grams of H and the grams of C from the 1 gram total, the remainder is O.
C = 2.90 g/1.00 g = 2.90 g/1.00 g x 100% = 290%
H = .875 g/1.00 g = .875 g/1.00 g x 100% = 87.5%
O = 1.00 g - 2.90 g - .875 g = .225 g/1.00 g x 100% = 22.5%
Well, looks like Testosterone is made up of some carbon, hydrogen, and oxygen. Let's find out the mass percents of each element!
First, we'll calculate the mass of carbon. We know that 2.90 g of CO2 contains the same mass of carbon. Since the molecular weight of CO2 is 12.01 g/mol for carbon and 44.01 g/mol for CO2, we can set up a simple ratio:
(2.90 g CO2) * (12.01 g C / 44.01 g CO2) = x grams of C
Simplifying that, we get:
x = 0.790 g of C
So, the mass percent of carbon in testosterone would be:
(0.790 g C / 1.00 g testosterone) * 100% = 79.0% C
Next, let's calculate the mass of hydrogen. We know that 0.875 g of H2O contains the same mass of hydrogen. The molecular weight of H2O is 18.02 g/mol, so:
(0.875 g H2O) * (2.02 g H / 18.02 g H2O) = y grams of H
Simplifying that, we get:
y = 0.097 g of H
So, the mass percent of hydrogen in testosterone would be:
(0.097 g H / 1.00 g testosterone) * 100% = 9.7% H
Finally, to find the mass percent of oxygen, we can subtract the total mass of carbon and hydrogen from the mass of testosterone:
Mass of oxygen = 1.00 g - 0.790 g (C) - 0.097 g (H) = 0.113 g
So, the mass percent of oxygen in testosterone would be:
(0.113 g O / 1.00 g testosterone) * 100% = 11.3% O
Therefore, the mass percents of carbon, hydrogen, and oxygen in testosterone are approximately 79.0% C, 9.7% H, and 11.3% O, respectively.
To calculate the mass percentages, divide the mass of each element by the total mass of testosterone (1.00g), then multiply by 100.
1. Calculate the mass percent of carbon:
Mass of carbon = mass of CO2 (2.90g) - mass of oxygen in CO2 (2.90g - (2 * atomic mass of oxygen))
Mass of carbon = 2.90g - (2 * 16.00g/mol) = 2.90g - 32.00g/mol = -29.10g/mol
To convert grams of carbon to mass percent, divide by the total mass of testosterone and multiply by 100:
Mass percent of carbon = (2.90g CO2 / 1.00g testosterone) * 100 = 290%
2. Calculate the mass percent of hydrogen:
Mass of hydrogen = mass of H2O (0.875g) - mass of oxygen in H2O (0.875g - (1 * atomic mass of oxygen))
Mass of hydrogen = 0.875g - (1 * 16.00g/mol) = 0.875g - 16.00g/mol = -15.125g/mol
To convert grams of hydrogen to mass percent, divide by the total mass of testosterone and multiply by 100:
Mass percent of hydrogen = (0.875g H2O / 1.00g testosterone) * 100 = 87.5%
3. Calculate the mass percent of oxygen:
Mass of oxygen = Total mass of testosterone (1.00g) - mass of carbon - mass of hydrogen
Mass of oxygen = 1.00g - (-29.10g/mol) - (-15.125g/mol) = 45.225g/mol
To convert grams of oxygen to mass percent, divide by the total mass of testosterone and multiply by 100:
Mass percent of oxygen = (45.225g / 1.00g testosterone) * 100 = 4522.5%
Therefore, the mass percents of carbon, hydrogen, and oxygen in testosterone are 290%, 87.5%, and 4522.5%, respectively.
To solve the problem, follow these steps:
Step 1: Determine the mass of carbon (C) in testosterone:
Given that 2.90 g of CO2 contain the same mass of carbon (C) as 1.00 g of testosterone, we can assume that all the carbon in testosterone is converted to CO2 during the combustion. Since the molar mass of CO2 is 44 g/mol, we can calculate the mass of carbon by multiplying the mass of CO2 by the ratio of the atomic masses of carbon to the molecular mass of CO2:
Mass of C = (2.90 g CO2) × (12.01 g C / 44.01 g CO2) = 0.789 g C
Step 2: Determine the mass of hydrogen (H) in testosterone:
Given that 0.875 g of H2O contain the same mass of hydrogen (H) as 1.00 g of testosterone, we can assume that all the hydrogen in testosterone is converted to H2O during the combustion. Since the molar mass of H2O is 18.02 g/mol, we can calculate the mass of hydrogen by multiplying the mass of H2O by the ratio of the atomic masses of hydrogen to the molecular mass of H2O:
Mass of H = (0.875 g H2O) × (2.02 g H / 18.02 g H2O) = 0.097 g H
Step 3: Determine the mass of oxygen (O) in testosterone:
The mass of oxygen can be obtained by subtracting the mass of carbon and hydrogen from the total mass of testosterone:
Mass of O = Total mass of testosterone - Mass of C - Mass of H
Mass of O = 1.00 g - 0.789 g - 0.097 g = 0.114 g O
Step 4: Calculate the mass percent of each element in testosterone:
To find the mass percent of each element, divide the mass of each element by the total mass of testosterone and multiply by 100:
Mass percent of C = (0.789 g C / 1.00 g of testosterone) × 100% = 78.9%
Mass percent of H = (0.097 g H / 1.00 g of testosterone) × 100% = 9.7%
Mass percent of O = (0.114 g O / 1.00 g of testosterone) × 100% = 11.4%
Therefore, the mass percents of carbon, hydrogen, and oxygen in testosterone are 78.9%, 9.7%, and 11.4% respectively.