If 42 grams of carbon in 52 grams of oxygen are used how many grams of CO2 will be produced. I need to show work.
1 answer:
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<u>Answer:</u> The vapor pressure of solution is 459.17 mmHg
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For testosterone:</u>
Given mass of testosterone = 7.752 g
Molar mass of testosterone = 288.4 g/mol
Putting values in equation 1, we get:
- <u>For diethyl ether:</u>
Given mass of diethyl ether = 208.0 g
Molar mass of diethyl ether = 74.12 g/mol
Putting values in equation 1, we get:
Mole fraction of a substance is calculated by using the equation:
The formula for relative lowering of vapor pressure will be:
where,
= vapor pressure of solvent (diethyl ether) = 463.57 mmHg
= vapor pressure of the solution = ?
i = Van't Hoff factor = 1 (for non electrolytes)
= mole fraction of solute (testosterone) = 0.0095
Putting values in above equation, we get:
Hence, the vapor pressure of solution is 459.17 mmHg