If a sample of 4 moles of gas has a pressure of 567.42 kPa and a volume of 12.0 L, what is its temperature?
It's -68 °C in there.
We can apply the Ideal Gas Law to provide an answer to this query:
The gas's temperature is -68 °C.
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Using the ideal gas law (PV = nRT), where (P) is pressure, (V) is volume, (n) is the number of moles, (R) is the gas constant, and (T) is temperature in Kelvin:
Given: (P = 567.42 , \text{kPa}) (V = 12.0 , \text{L}) (n = 4 , \text{mol})
We can rearrange the equation to solve for temperature: [T = \frac{{PV}}{{nR}}]
Using the ideal gas constant (R = 8.314 , \text{J/(mol·K)}):
[T = \frac{{567.42 \times 12.0}}{{4 \times 8.314}}]
[T ≈ 204.7 , \text{K}]
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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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