Question

I need help on 4.8 and 4.9. Will I use the Ideal Gas Law for 4.8 or use another one? As for 4.9 would I use Boyle’s or Avogadro’s law?

Thank you!!!

Calculate the volume occupied by 1.5 moles of an ideal gas at 25°C and a pressure of 0.80 atm. (R = 0.08206 L. atm/(mol-K). 4.8 A sample of carbon monoxide has a volume of 150 mL at 10. °C and 0.75 atm. What pressure will be exerted by the gas if the temperature is increased to 522 C and the volume changed to 500. mL? 4.9 4-25

Answer 1

Ans 4.8 :

We will use the ideal gas law , pV = nRT

T = 25 degrees C = 298.15 K

p = 0.80 atm

n = 1.5 moles

Putting all the values in law , we get :

0.80 x V = 1.5 x 0.08206 x 298.15

V = 45.9 L

So the volume occupied will be 45.9 L

Ans 4.9 :

Using the ideal gas law , pV = nRT , we get the relation : p1V1 T2 = p2V2 T1

p1 = 0.75 atm

V1 = 150 mL = 0.150 L

T1 = 10 degrees C = 283.15 K

p2 = ?

V2 = 500 mL = 0.500 L

T2 = 522 degrees C = 795.15 K

So putting all the values we get :

0.75 x 0.150 x 795.15 = p2 x 0.500 x 283.15

p2 = 0.632 atm

So the pressure exerted by the gas will be 0.632 atm.