A student following the procedure described in this experiment collected the following data:

Mass Mg,g 0.0243
volume of gas mL 25.5
barometric pressure, mm Hg 298
Calculate the value of the gas law constant, R.
Please help me work this out, I have no idea. Thank you!

Surely you haven't typed all of the question. What gas is collected? Is it collected over water or not. What is the temperature? The pressure surely is not 298 mm Hg.

Use PV = nRT.
P = (mmHg - mmHg vapor pressure H2O/760)
V = 0.0255
n = 24.3/atomic mass Mg
R = solve for this
T = 273 + celsius.

To calculate the gas law constant, R, you need to use the ideal gas law equation, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature.

In this case, the given data includes the following:
Pressure: 298 mm Hg
Volume: 25.5 mL
Mass of Mg: 0.0243 g

To calculate the number of moles of gas (n), you can use the molar mass of magnesium (Mg), which is about 24.31 g/mol.

n = mass of Mg / molar mass of Mg
n = 0.0243 g / 24.31 g/mol

Next, convert the given volume from milliliters (mL) to liters (L) since the gas constant is typically expressed in liters (L).

Volume = 25.5 mL = 0.0255 L

Now, we can rearrange the ideal gas law equation to solve for R:
R = PV / (nT)

Substitute the given values into the equation:
R = (Pressure) * (Volume) / (number of moles of gas * Temperature)

R = (298 mm Hg) * (0.0255 L) / (0.0243 g / 24.31 g/mol * Temperature)

The final step is to calculate the value of R by plugging in the values:
R = (298 mm Hg) * (0.0255 L) / (0.0243 g / 24.31 g/mol * Temperature)

Please note that the temperature is missing in the given data, so you will need to provide the temperature in order to calculate the gas law constant, R.