Oh my.

We will make our initial calculations using $PV=nRT$ , and then solve for variables to plug into $W=nRT*ln(\frac{V_f}{V_i})$ . Since we're calculating the answer in Joules and using Kelvin, we'll use the gas constant R in units of J/mol*K.

$R=8.314 ^\text{ J}/_\text{ mol K}$ .

$P_i = 1$ atm

$n = ^\text{ g of Oxygen}/_\text{ atomic mass of Oxygen} = \frac{24g}{15.999g/mol} \rightarrow n=1.500\text{ mols}$

$T=298$ K

Solving for $V_i$ by plugging these values into $PV=nRT$ gives...

$(1 atm)V_i = (1.500)(8.314)(298) \rightarrow V_i=36.68$

So, now that we know the initial Volume, we can calculate the final Volume using the final Pressure $P_f = 50$ atm.

$(50 atm)V_f = (1.500)(8.314)(298) \rightarrow V_f=0.7337$

Now we can plug these into $W=nRT*ln(\frac{V_f}{V_i})$ to find the work.

Solving for W gives: $W\approx-7270.55 J$

keep on adding Chemistry questions. We have very few peoples in Brilliant who post chemistry questions