If #24 L# of a gas at room temperature exerts a pressure of #72 kPa# on its container, what pressure will the gas exert if the container's volume changes to #7 L#?
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Using the combined gas law (PV/T = \text{constant}), where (P) is pressure, (V) is volume, and (T) is temperature, and assuming constant temperature:
[ P_1V_1 = P_2V_2 ]
[ (72 \ \text{kPa})(24 \ \text{L}) = P_2(7 \ \text{L}) ]
[ P_2 = \frac{(72 \ \text{kPa})(24 \ \text{L})}{7 \ \text{L}} ]
[ P_2 \approx 248 \ \text{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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