How do I do numbers 3 and 4 for gas laws Ideal Gas Law QuI2

Ideal Gas Law QuI2 If this item does not open automatically you can open Ideal Gas Law Quiz here PV nRT 1/2 3. What pressure will be exerted by 25 g of CO2 at a temperature of 25 °C and a volume of 500. mL? 4. At what temperature will 5.00 g of Cl2 exert a pressure of 900. torr at a volume of 750. mL? 5. What is the density of NH3 at 800. torr and 25 °C? DOL

Solution

From Gas laws we know that ,

  PV = nRT Where P is Pressure , V is Volume , n is the number of moles , T is temperature and R is the universal Gas Constant .   R = 0.082 L-atm mol^-1 K^-1

R = 62.363 L-torr mol^-1 K^-1

1 @ given 25 g of CO₂ , since molar mass of  CO₂ is 44 g , then 25 g of CO₂ contains 25 / 44 moles or   0.568 moles . volume is 0.5 L and Temperature is 298 K , the the pressure will be :

P = ( nRT / V ) = ( 0.568 x 0.082 x 298 ) / 0.5 =  27.76 atm

2 @

Given , 5 g of Cl₂ , since molar mass of Cl₂is  70.906 g ,then 5 g of Cl₂contains 5 / 70.906 moles or 0.07051 moles of Cl₂exerts a pressure of 900 torr in a volume of 0.75 L , then the temperature of the gas will be

  T = PV / nR , where   R = 62.363 L-torr mol^-1 K^-1

then T = ( 900 x 0.75 ) / ( 0.07051 x 62.363 ) = 153.506 K

3 @

since ,     PV = nRT    P = ( n / V ) RT ; where \' n \' is the number of moles since , n = ( mass of the gass / molar mass of the gass ) since , ( Mass of the gas / Volume of gas ) = density of the gas ( d )

then , P = (dRT / molar mass of the gass )

d = ( P x molar mass of the gass ) / RT  

Ammonia ( NH₃ ) gas is given whose molar mass 17.031 g exerting a pressure of 800 torr at 298 K then the density of the gas will be

  d = ( P x molar mass of the gass ) / RT   , where R = 62.363 L-torr mol^-1 K^-1

   d = ( 800 x 17.031 ) / 62.363 x 298 = 0.733 g / L