Hello, Reyes,
Use the ideal gas law equation:
PV=nRT
where P is the pressure, V is the volume, n is the moles, R is the gas constant, and T is the temperature in Kelvin. The gas constant should be in your book, or notes. I picked the constant that matches the units givien (L, atm, K, and moles):
| 0.082057366080960 | L⋅atm⋅K−1⋅mol−1 |
For ease, rearrange the equation to separate T from the rest:
T = PV/nR
Now input the date: T(K) = (11atm*0.042L)/(0.77mole*0.082057L*atm*K-1mol-1)
Atmospheres, moles, and liters cancel and Kelvin moves to the top. I get 7.3K, to two sig figs. Seems low, so check the calculations. Especially check the gas constant given by the book. I got mine from Wikipedia, so who knows?
Bob
