Question

If a gas is compressed from 4L to 1L, and the temperature remains constant, what happens to the pressure?

Answer 1

USING BOYLE'S  LAW PRESSURE BECOMES 4 TIMES WHEN GAS IS COMPRESSED WITHOUT TEMPERATURE CHANGE.

Explanation:

In a container having 4L there are bunch of molecules bouncing around walls and this movement of molecules indicates pressure in the container.

Logically to see when the gas is compressed from 4L to 1L it shows the increased amount of pressure over the container as the number of gas molecules increased and the collisions also increase as the container is same and pressure increases.

Use the equation:

(P1 * V1) / T1 = (P2 * V2) / T2

now cross-multiplying to get

P1 * V1 * T2 = P2 * V2 * T1

Replace V1 with 4L and V2 with 1L. Also, Temperature remains constant, so taking it out of the equation

P1 * 4L = P2 * 1L

Divide both sides by 1L:

P1 * 4 = P2

So the end pressure will be 4 times the beginning pressure.

Answer 2

If a gas is compressed from 4L to 1L, and the temperature remains constant then  the end pressure will be 4 times the beginning pressure.

Pressure after changing volume at a constant temperature

• We know initial volume = 4L
• After compression = 1 L

By the Charles and Boyles law from the ideal gas equation:

$\frac{(P_1 \times V_1)}{T_1} = \frac{(P_2 \times _2)}{T_2}$

As we have Volume initially with 4L and volume after compression 1L. Also, Temperature remains constant, so taking it out of the equation

$P_1 *\times 4L = P_2 *\times 1L$

Divide both sides by 1L:

$P_1 * 4 = P_2$

So the end pressure will be 4 times the beginning pressure.

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