Helium in a 100 mL container at a pressure of 66.6 kPa is transferred to a container with a volume of 250 mL. What is the new pressure if no change in temperature occurs?
For this problem we would us the equation for Boyle's Law comparing the inverse relationship between pressure and volume when the temperature is held constant.
First we would determine ore known and unknown values from the question.
The equation can be rearranged algebraically to I hope this was helpful.
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To find the new pressure when transferring helium from a 100 mL container to a 250 mL container with no change in temperature, we use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when temperature remains constant.
Boyle's Law formula: P1 * V1 = P2 * V2
Where: P1 = initial pressure (66.6 kPa) V1 = initial volume (100 mL) P2 = final pressure (unknown) V2 = final volume (250 mL)
Substituting the given values into the formula:
66.6 kPa * 100 mL = P2 * 250 mL
To find P2, rearrange the equation:
P2 = (66.6 kPa * 100 mL) / 250 mL
P2 ≈ 26.64 kPa
Therefore, the new pressure is approximately 26.64 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.
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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