How many O2 molecules occupy a 1.0 L flask at 65oC and103.7 kPa?Question 4Select one:a.28 moleculesb.2.2 x 1022 moleculesc.1.1 x 1023 moleculesd.1.6 x 1025 moleculese.1.7 x 1025 molecules

To solve this problem, we can use the Ideal Gas Law, which states that the pressure of a gas times its volume is equal to the number of moles of the gas times the ideal gas constant times the temperature of the gas (in Kelvin). The formula is PV = nRT.

First, we need to convert the given temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = C + 273.15. So, 65°C = 65 + 273.15 = 338.15 K.

Next, we need to convert the pressure from kilopascals to atmospheres because the ideal gas constant (R) we are using is in terms of atmospheres. The conversion factor is 1 atm = 101.325 kPa. So, 103.7 kPa = 103.7/101.325 = 1.023 atm.

Now we can plug these values into the Ideal Gas Law and solve for n (the number of moles):

1.023 atm * 1.0 L = n * 0.0821 Latm/molK * 338.15 K

Solving for n gives us n = 0.0375 mol.

Finally, we need to convert moles to molecules. The conversion factor is 1 mol = 6.022 x 10^23 molecules. So, 0.0375 mol = 0.0375 * 6.022 x 10^23 = 2.26 x 10^22 molecules.

So, the closest answer is b. 2.2 x 10^22 molecules.