What volume is needed to store 0.80 moles of helium gas at 204.6 kPa and 300 K?
The volume of helium gas is
Now what you want to do is list your known and unknown variables. Our only unknown is the volume of helium gas. Our known variables are P,n,R, and T.
The pressure has the incorrect units because the pressure should be in atmospheres instead of kPa. In order to go from kPa to atm we use the following relationship:
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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:
( V = \frac{nRT}{P} = \frac{(0.80 \text{ mol})(8.31 \text{ kPa} \cdot \text{L/mol} \cdot \text{K})(300 \text{ K})}{204.6 \text{ kPa}} )
( V \approx 9.19 \text{ 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.
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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