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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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    Solution Preview

    (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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