A sample of neon gas is stored in a 
\[5.0\text{-L}\] metal cylinder at a pressure of 
\[175\text{ atm}\]. The gas is then transferred to a larger container with a volume of 
\[12\text{ L}\]. The temperature of the gas remains constant.
several large metal, gray and white cylinders used to hold pressurized gases
Metal cylinders containing pressurized gases
Calculate the pressure of the neon gas in the new container.
Round your answer to the nearest whole number.
 
\[\text{atm}\]
 
 
 
 
 
 
 












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.

A sample of neon gas is stored in a [5.0-L] metal cylinder at a pressure of [175 atm]. The gas is then transferred to a larger container with a volume of [12 L]. The temperature of the gas remains constant. Calculate the pressure of the neon gas in the new container. Round your answer to the nearest whole number.

Learn how to calculate the pressure of neon gas when transferred to a larger container using Boyle's Law. This problem explores the relationship between gas pressure and volume under constant temperature. Suitable for high school students in Grades 9-12.

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