To solve this, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when the temperature and the amount of gas are constant. Boyle's Law is expressed as:

$P_1 V_1 = P_2 V_2$

Where:

• $P_1$ is the initial pressure,
• $V_1$ is the initial volume,
• $P_2$ is the final pressure, and
• $V_2$ is the final volume.

Given values:

• $P_1 = 175\text{ atm}$,
• $V_1 = 5.0\text{ L}$,
• $V_2 = 12\text{ L}$.

We need to find $P_2$, the pressure in the new container. Rearranging Boyle's Law to solve for $P_2$:

$P_2 = \frac{P_1 V_1}{V_2}$

Now, let's calculate the final pressure $P_2$:

$P_2 = \frac{175 \times 5.0}{12}$

$P_2 \approx 72.92 \text{ atm}$

Rounding to the nearest whole number:

$P_2 \approx 73 \text{ atm}$

Thus, the pressure of the neon gas in the new container is 73 atm.

Would you like further details or have any questions?

Here are 5 related questions to expand on this:

1. How does Boyle's Law apply to real-world gas storage systems?
2. What happens to gas pressure when both volume and temperature change?
3. How does neon behave differently from other gases in terms of ideal gas law?
4. Why does Boyle's Law require constant temperature for accuracy?
5. How does increasing container size impact gas pressure in everyday applications?

Tip: Always check if temperature remains constant when applying Boyle's Law, as it's crucial for accuracy.