A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the

pressure is increased to 894 torr at constant temperature?

Well, if nitrogen gas were a person, it would definitely feel a little squished under all that pressure! But luckily, gases are quite flexible.

To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. So, if we keep the temperature constant, we can use the formula:

P1V1 = P2V2

Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Plugging in the values we have:
P1 = 745 torr
V1 = 37.42 L
P2 = 894 torr
V2 = ?

Using the formula, we can rearrange it to find V2:

V2 = (P1 * V1) / P2

V2 = (745 torr * 37.42 L) / 894 torr

Calculating that out, we find the volume will be approximately 31.07 L.

So, to answer your question, if the pressure of the nitrogen gas is increased to 894 torr at the same temperature, it will occupy a volume of 31.07 L. Just enough room to stretch its gas molecules a bit!

To solve this problem, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure, as long as the temperature remains constant.

The formula for Boyle's Law is:

P1 * V1 = P2 * V2

Where:
- P1 is the initial pressure (745 torr)
- V1 is the initial volume (37.42 L)
- P2 is the final pressure (894 torr)
- V2 is the final volume (what we need to find)

Let's substitute the known values into the formula and solve for V2:

(745 torr) * (37.42 L) = (894 torr) * V2

Now, we can solve for V2:

V2 = (745 torr * 37.42 L) / 894 torr

V2 = 31.10 L

Therefore, the volume of the nitrogen gas will be 31.10 L when the pressure is increased to 894 torr at constant temperature.

To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. The formula for Boyle's Law is:

P1 * V1 = P2 * V2

where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Now let's plug in the given values into the equation:

P1 = 745 torr
V1 = 37.42 L
P2 = 894 torr (the pressure is increased to this value)
V2 = ?

To find V2, we rearrange the formula:

V2 = (P1 * V1) / P2

Substituting the values:

V2 = (745 torr * 37.42 L) / 894 torr

Now, let's calculate:

V2 = 30.985 L

Therefore, the volume of the nitrogen gas will be approximately 30.985 L when the pressure is increased to 894 torr at constant temperature.

P1

P1V1 = P2V2