At 27 degrees celcius, nitrogen has a volume of 650 cm^3 under a pressure of 980 mmHg. What would be its volume at the same temperature but at a pressure of 760 mmHg?

P1V1 = P2V2

Substitute and solve for the unknown.

To determine the volume of nitrogen at a new pressure, we can use Boyle's Law, which states that the product of pressure and volume for a given amount of gas is constant, as long as the temperature remains constant.

Boyle's Law can be expressed as: P1*V1 = P2*V2

Where,
P1 = initial pressure
V1 = initial volume
P2 = final pressure
V2 = final volume

In this particular problem, we are given:
P1 = 980 mmHg (initial pressure)
V1 = 650 cm^3 (initial volume)
P2 = 760 mmHg (final pressure)

To find V2, we rearrange the Boyle's Law equation:

V2 = (P1 * V1) / P2

Plugging in the given values:

V2 = (980 mmHg * 650 cm^3) / 760 mmHg

Now, for proper unit conversion, we need to convert mmHg to cm^3. Since 1 mmHg is equal to 1 cm^3, we don't need to make any conversions:

V2 = (980 * 650) / 760 cm^3

Simplifying further, we can calculate:

V2 ≈ 839.47 cm^3

Therefore, the volume of the nitrogen at the same temperature but at a pressure of 760 mmHg would be approximately 839.47 cm^3.