# A nitrogen gas occupies a volume of 500 ml at a pressure of 0.971 atm. What volume will the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?

This is a straightforward use of Boyle's law.

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Using Boyle's Law, ( P_1 \cdot V_1 = P_2 \cdot V_2 ), where ( P_1 ) and ( V_1 ) are the initial pressure and volume, and ( P_2 ) and ( V_2 ) are the final pressure and volume:

( 0.971 , \text{atm} \cdot 500 , \text{ml} = 1.50 , \text{atm} \cdot V_2 )

( V_2 = \frac{0.971 , \text{atm} \cdot 500 , \text{ml}}{1.50 , \text{atm}} )

( V_2 = 324.33 , \text{ml} ) (rounded to two decimal places)

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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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