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volume of oxygen

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(Problem 1) A person accidentally swallows a drop of liquid oxygen, O2(l), which has a density of 1.149 g/mL. Assuming the drop has a volume of 0.050 mL, what volume of gas will be produced in the person's stomach at body temperature (37 C) and a pressure of 1.0 atm?

(Problem 2 ) The density of N2O at 1.53 atm and 45.2 degrees celsius is how many grams per liter? I am setting up the formula but I cannot get the correct choice from multiple choice. I keep getting 7.04. I know I need to convert the celsius to Kelvin so that is not it. Can you help?

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(Problem 1) A person accidentally swallows a drop of liquid oxygen, O2(l), which has a density of 1.149 g/mL. Assuming the drop has a volume of 0.050 mL, what volume of gas will be produced in the person's stomach at body temperature (37 C) and a pressure of 1.0 atm?

Response:

First, we can determine the mass of the liquid oxygen.

(1.149 g/ml)(0.050 ml) = 0.05745 g

Now, we can convert this amount of oxygen into moles using ...

Solution Summary

It provides two examples of finding the volumes of the gas by applying the ideal gas law.

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Volume of oxygen required for the combustion of octane

Combustion Reactions

Combustion reactions are classified as rapid reactions that produce a flame. Usually, a combustion reaction refers to the reaction of a substance with O2.

A very important class of reactions is the combustion of hydrocarbons (compounds containing hydrogen and oxygen) to form CO2 and H2O.

All of the carbon in the sample is converted to CO2
All of the hydrogen in the sample is converted to H2O

Combustion of octane (C8H18) is the primary reaction in an automobile engine.

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