Answer:
141C
Explanation:
We need to use the ideal gas law to solve this question. Ideal gas law: PV = nRT
P = pressure = 4.00 atm = 4.00 × 101.325 = 405.3 kPa (pressure needs to be converted to kilopascals)
V = volume = 4.25L
n = number of moles = 0.500
R = gas constant = 8.314 mol/K (found om chemistry data sheet)
T = temperature = ? unknown
Before any other steps are taken, we need to rearrange the the ideal gas law formula to make T the subject.
PV/nR = T
Now we can substitute the values.
(405.3 × 4.25) ÷ (0.500 × 8.314) = 414.3673322107 (answer in kelvin)
Convert 414.3673322107 Kelvin to Celsius.
0C = 273.15K (found on chemistry data sheet)
414.3673322107 - 273.15 = 141.2173322107C
141.2173322107 to nearest C = 141C
