# If #8 L# of a gas at room temperature exerts a pressure of #2 kPa# on its container, what pressure will the gas exert if it the container's volume changes to #1 L#?

The final pressure is

Let's identify the known and unknown variables:

- Initial Volume

- Final Volume

- Initial Pressure

- Final Pressure

We can obtain the answer using Boyle's Law:

The letters i and f represent the initial and final conditions, respectively.

All we have to do is rearrange the equation to solve for the final pressure.

We do this by dividing both sides by

Now all we do is plug in the values and we're done!

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The pressure of the gas will be 16 kPa.

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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.

- If #3/7 L# of a gas at room temperature exerts a pressure of #12 kPa# on its container, what pressure will the gas exert if the container's volume changes to #5/4 L#?
- A container with a volume of #6 L# contains a gas with a temperature of #720^o K#. If the temperature of the gas changes to #420^o K# without any change in pressure, what must the container's new volume be?
- If #10/3 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#?
- How do buoyant forces occur?
- A sample of an ideal gas is stored at 21 degrees Celsius. To what temperature would it have to be heated to double the volume of the gas?

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