A 1.50 liter flask at a temperature of 25°C contains a mixture of 0.158 moles of methane, 0.09 moles of ethane, and 0.044 moles of butane. What is the total pressure of the mixture inside the flask?
Applying the general gas equation : PV=nRT V = 1.50 litres R = 0.08205746 L atm/K mol T = 25°C = 25+273 = 298 K n = 0.158 moles+0.09 moles+ 0.044 moles = 0.292 moles Re arranging the equation: P = nRT / V = (0.158 + 0.09 + 0.044) mol x (0.08205746 L atm/K mol) x
(25 + 273)K / (1.50 L) = 4.76 atm = 482 kPa = 3617 mmHg
