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Question: 1 / 400

A gas has an initial volume of 10 lt and pressure of 4 atm. If its volume becomes 20 lt, what will its final pressure be in cm-Hg?

152 cm-Hg

38 cm-Hg

To determine the final pressure of the gas when its volume changes, we can use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume when the temperature remains constant. This can be mathematically expressed as:

\[ P_1 \times V_1 = P_2 \times V_2 \]

Where:

- \( P_1 \) is the initial pressure.

- \( V_1 \) is the initial volume.

- \( P_2 \) is the final pressure.

- \( V_2 \) is the final volume.

In this scenario:

- The initial volume \( V_1 \) is 10 liters.

- The initial pressure \( P_1 \) is 4 atm.

- The final volume \( V_2 \) is 20 liters.

Using Boyle's Law, we can substitute in the values:

\[ 4 \, \text{atm} \times 10 \, \text{lt} = P_2 \times 20 \, \text{lt} \]

Next, solve for \( P_2 \):

\[ P_2 = \frac{(4 \, \text{atm} \times 10 \

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76 cm-Hg

2 cm-Hg

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