To solve this problem, you will need to use the ideal gas law, which relates the volume, temperature, and pressure of a gas to the number of moles of gas present. Specifically, the ideal gas law is given by the equation PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in kelvins.
Since the volume of the gas is given in liters and the temperature is given in kelvins, the ideal gas law can be written in the form PV = nRT, where R = 8.31 L atm/mol K.
First, you need to determine the mass of H2S present in the sample of natural gas. The sample contains 0.070% H2S by volume, which means that 0.070% of the sample is H2S and the rest is other gases. If the mass of the sample is m, then the mass of H2S present in the sample is 0.070/100 * m = 0.00070m.
Next, you need to determine the number of moles of H2S present in the sample. The molar mass of H2S is 34.08 g/mol, so the number of moles of H2S present in the sample is 0.00070m / 34.08 g/mol = 2.05 x 10^-5 moles.
Finally, you need to determine the mass of H2S present in 2.00 L of natural gas at 298 K. Since the volume and temperature of the natural gas are given, you can use the ideal gas law to solve for the number of moles of gas present:
PV = nRT
n = PV / RT
Substituting the given values and solving for n, we find that n = 2.00 L * 101325 Pa / (8.31 L atm/mol K * 298 K) = 0.038 moles
Since the number of moles of H2S present in the sample is 2.05 x 10^-5 moles, this means that the mass of H2S present in 2.00 L of natural gas at 298 K is 0.038 moles * 34.08 g/mol = 1.32 g.
Therefore, the mass of H2S present in 2.00 L of natural gas at 298 K is 1.32 g.