# An emphysema patient is breathing pure O2 through a face mask. The cylinder of O2 contains 0.60 ft3 of O2 gas at a pressure of 2300 lb/in2. What volume would the oxygen occupy at atmospheric pressure (and the same temperature)?

The volume of oxygen would be

It looks like there is a Boyle's Law issue here.

Boyle's Law states

Boyle's Law can be rearranged to get

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To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when the temperature and the amount of gas are constant.

P1 * V1 = P2 * V2

Where: P1 = Initial pressure V1 = Initial volume P2 = Final pressure V2 = Final volume

We are given: P1 = 2300 lb/in^2 V1 = 0.60 ft^3 P2 = 14.7 lb/in^2 (atmospheric pressure)

Rearranging the equation for V2, we get:

V2 = (P1 * V1) / P2

Plugging in the values:

V2 = (2300 lb/in^2 * 0.60 ft^3) / 14.7 lb/in^2

V2 ≈ 93.88 ft^3

So the volume of oxygen at atmospheric pressure would be approximately 93.88 ft^3.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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