Sure, let's solve this step by step.

This problem can be solved using Boyle's law, which states that the pressure and volume of a gas have an inverse relationship when temperature is held constant. In other words, if the pressure increases, the volume decreases and vice versa.

In this case, the initial volume (V1) is 400 cm^3 and the initial pressure (P1) is 5 times the atmospheric pressure. We want to find the final volume (V2) when the gas is released to atmospheric pressure (P2).

Boyle's law is expressed as P1*V1 = P2*V2.

We know P1 (5 times atmospheric pressure), V1 (400 cm^3), and P2 (atmospheric pressure). We want to find V2.

So, we rearrange the formula to solve for V2: V2 = P1*V1 / P2.

Substituting the known values into the equation gives us: V2 = 5 * 400 cm^3 / 1 = 2000 cm^3.

So, the volume that the air would occupy if it were all released to atmospheric pressure is 2000 cm^3.

Question

Sure, let's solve this step by step.

This problem can be solved using Boyle's law, which states that the pressure and volume of a gas have an inverse relationship when temperature is held constant. In other words, if the pressure increases, the volume decreases and vice versa.

In this case, the initial volume (V1) is 400 cm^3 and the initial pressure (P1) is 5 times the atmospheric pressure. We want to find the final volume (V2) when the gas is released to atmospheric pressure (P2).

Boyle's law is expressed as P1*V1 = P2*V2.

We know P1 (5 times atmospheric pressure), V1 (400 cm^3), and P2 (atmospheric pressure). We want to find V2.

So, we rearrange the formula to solve for V2: V2 = P1*V1 / P2.

Substituting the known values into the equation gives us: V2 = 5 * 400 cm^3 / 1 = 2000 cm^3.

So, the volume that the air would occupy if it were all released to atmospheric pressure is 2000 cm^3.

Knowee AI · Accepted Answer

Sure, let's solve this step by step.

This problem can be solved using Boyle's law, which states that the pressure and volume of a gas have an inverse relationship when temperature is held constant. In other words, if the pressure increases, the volume decreases and vice versa.

In this case, the initial volume (V1) is 400 cm^3 and the initial pressure (P1) is 5 times the atmospheric pressure. We want to find the final volume (V2) when the gas is released to atmospheric pressure (P2).

Boyle's law is expressed as P1*V1 = P2*V2.

We know P1 (5 times atmospheric pressure), V1 (400 cm^3), and P2 (atmospheric pressure). We want to find V2.

So, we rearrange the formula to solve for V2: V2 = P1*V1 / P2.

Substituting the known values into the equation gives us: V2 = 5 * 400 cm^3 / 1 = 2000 cm^3.

So, the volume that the air would occupy if it were all released to atmospheric pressure is 2000 cm^3.

The can has a volume of 400 cm ^3 and the pressure of the compressed air inside is 5 times atmospheric pressure. Calculate the volume that the air would occupy if it were all released to atmospheric pressure

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