What mass of CH4 would take up 24.790 L at 25 °C and 1 bar?Group of answer choices16 g24 g12 g20 g

To solve this problem, we need to use the ideal gas law equation, which is PV = nRT.

Here, P = pressure = 1 bar = 1.01325 atm (since 1 bar = 1.01325 atm) V = volume = 24.790 L R = gas constant = 0.0821 L.atm/mol.K T = temperature = 25 °C = 298.15 K (since 273.15 + 25 = 298.15)

We need to find n, the number of moles of CH4.

Rearranging the ideal gas law equation to solve for n, we get n = PV/RT.

Substituting the given values, we get n = (1.01325 * 24.790) / (0.0821 * 298.15) = 1.01325 mol.

The molar mass of CH4 is approximately 16 g/mol.

Therefore, the mass of CH4 is n * molar mass = 1.01325 mol * 16 g/mol = 16.212 g.

Rounding to the nearest whole number, we get approximately 16 g.

So, the answer is 16 g.