# If #15/4 L# of a gas at room temperature exerts a pressure of #42 kPa# on its container, what pressure will the gas exert if the container's volume changes to #12/7 L#?

The new pressure is

Utilize Boyle's Law.

The last bit of pressure is

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Using Boyle's Law, P1V1 = P2V2:

(42 kPa) * (15/4 L) = P2 * (12/7 L)

P2 = (42 kPa) * (15/4 L) / (12/7 L)

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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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- A container with a volume of #32 L# contains a gas with a temperature of #240^o K#. If the temperature of the gas changes to #160 ^o K# without any change in pressure, what must the container's new volume be?
- A container has a volume of #48 L# and holds #6 mol# of gas. If the container is compressed such that its new volume is #36 L#, how many moles of gas must be released to maintain a constant temperature and pressure?
- A container with a volume of #14 L# contains a gas with a temperature of #160^o C#. If the temperature of the gas changes to #320 ^o K# without any change in pressure, what must the container's new volume be?

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