.Answer:
The gas constant has a value of 0.082 L*atm/mol*K
Explanation:
Step 1: Data given
Temperature = 25.0 °C = 298.15 K
Number of moles O2 gas = 1.00 moles
Volume = 12.5 L
Pressure = 198 Kpa = 1.95411 atm
Step 2: Calculate the gas constant
p*V = n*R*T
⇒with p = the pressure of the gast = 1.95411 atm
⇒with V = the volume of the gas = 12.5 L
⇒with n = the number of moles of O2 gas = 1.00 moles
⇒with R = the gas constant = TO BE DETERMINED
⇒with T = the temperature = 25 °C = 298.15 K
R = (p*V) / (n*T)
R = (1.95411 * 12.5) / (1.00 * 298.15)
R = 0.082 L*atm*mol*K
The gas constant has a value of 0.082 L*atm/mol*K
Answer:
8.305 L.KPa/mol.K
Explanation:
Step 1:
Data obtained from the question. This includes:
Temperature (T) = 25°C
Number of mole (n) = 1 mole
Volume (V) = 12.5 L
Pressure (P) = 198 KPa
Gas constant (R) =?
Step 2:
Conversion of celsius temperature to Kelvin temperature. This is illustrated below:
K = °C + 273
K = 25°C + 273
K = 298K
Therefore, the temperature is 298K
Step 3:
Determination of the gas constant.
Applying the ideal gas equation PV = nRT, the gas constant can be obtained as follow:
PV = nRT
198KPa x 12.5L = 1mol x R x 298K
Divide both side 1mol x 298K
R = (198KPa x 12.5L) / (1mol x 298K)
R = 8.305L.KPa/mol.K
Therefore the gas constant is 8.305L.KPa/mol.K
