# A container has a volume of #72 L# and holds #6 mol# of gas. If the container is compressed such that its new volume is #3 L#, how many moles of gas must be released to maintain a constant temperature and pressure?

Applying Avogadro's law here:

The initial conditions are denoted by the number 1, and the final conditions are represented by the number 2.

• Determine the variables you know and don't know:

• Rewrite the equation to find the total number of moles in the end:

• Enter the provided values to determine the total number of moles:

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Using the ideal gas law, we can solve for the number of moles of gas released. According to Avogadro's law, at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of gas present. So, we can set up the equation:

( \frac{V_1}{n_1} = \frac{V_2}{n_2} )

Given that (V_1 = 72 , \text{L}), (n_1 = 6 , \text{mol}), and (V_2 = 3 , \text{L}), we can solve for (n_2):

( \frac{72}{6} = \frac{3}{n_2} )

( \frac{72}{6} = \frac{3}{n_2} )

( n_2 = \frac{3 \times 6}{72} = \frac{1}{4} )

So, ( n_2 = 1.5 , \text{mol} )

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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.

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