I need to know the formulas and each step of how to work theseout so I can do others like this Thanks! The pressure of hydrogen gas in a constant-volume cylinder is2.25 atm at 0C. What will the pressure be if the temperature israised to 80 C? What would 905 g of Nitrogen gas N2 occupy at 200K and 2.0atm? I need to know the formulas and each step of how to work theseout so I can do others like this Thanks! The pressure of hydrogen gas in a constant-volume cylinder is2.25 atm at 0C. What will the pressure be if the temperature israised to 80 C? What would 905 g of Nitrogen gas N2 occupy at 200K and 2.0atm?
Explanation / Answer
From gas law PV = nRT Since volume is kept constant P T P / P' = T / T ' P = Initial pressure = 2.25 atm P' = final pressure = ? T = Initial temp. = 0 o C = 273 K T' = Final temp. = 80 o C = 80 + 273 = 353 K So, P' = PT' / T = (2.25 * 353) / 273 = 2.91atm PV = nRT = (w/M ) RT Where P = pressure = 2 atm w= mass of Nitrogen = 905 g M= mol. wt. of Niotrogen = 28 g T= temperature in Kelvin = 200 K V= volume of the gas = ? So,V = wRT / MP = ( 905 g * 0.0821L atm /mol-K * 200K ) / ( 28 g * 2 atm) = 265.35L