A sample of nitrogen (N2) gas has a volume of 250ml at 30 degrees C and a pressure of 745mmHg. What is the volume of the nitrogen at STP?

I got 22 liters in significant figures is this right. thank you.

If you post your work someone will try to find the error. I obtained something like 221 mL, a far cry from 22 L.

To find the volume of nitrogen at STP (Standard Temperature and Pressure), we need to use the ideal gas law equation, which states:

PV = nRT

Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

First, we need to convert the given values to the proper units. The temperature should be in Kelvin (K), and the pressure should be in atmospheres (atm). We can use the following conversions:

°C to K: K = °C + 273.15
mmHg to atm: atm = mmHg / 760

Using these conversions, we find:
Temperature (in Kelvin): T = 30 + 273.15 = 303.15 K
Pressure (in atm): P = 745 mmHg / 760 = 0.9789 atm

Now, the conditions at STP are:
- Temperature (in Kelvin): T = 273.15 K
- Pressure (in atm): P = 1 atm

We can rearrange the ideal gas law equation to solve for the volume at STP:
V (STP) = (nRT) / P (STP)

Since we're given the volume and conditions for the sample, we don't have enough information to calculate the number of moles (n) directly. However, we can use the fact that the volume of a gas is directly proportional to the number of moles of that gas, assuming constant temperature and pressure. This allows us to set up a ratio and solve for the volume at STP:

(V initial) / (n initial) = (V STP) / (n STP)

Substituting the values:
250 ml / n = V (STP) / 1

We need to find 'n' from the given sample, and since nitrogen gas (N2) has a molar mass of 28 g/mol, we can use the following formula to calculate the number of moles:

n = mass / molar mass

Unfortunately, the mass of the sample is not given in the question. Without the mass, we cannot determine the number of moles and subsequently calculate the volume at STP.

Therefore, it is not possible to confirm if your initial answer of 22 liters (since it is in significant figures) is correct without knowing the mass of the sample.