Answer:
final pressure ( P2) = 467.37 mm Hg
Explanation:
ideal gas:
∴ P1 = 570 mm Hg * ( atm / 760 mm Hg ) = 0.75 atm
∴ T1 = 25 ° C = 298 K
∴ V1 = 1.250 L
∴ R = 0.082 atm L / K mol
⇒ n = P1*V1 / R*T1
⇒ n = (( 0.75 ) * ( 1.25 )) / (( 0.082 ) * ( 298 ))
⇒ n = 0.038 mol gas
∴ T2 = 175 °C ( 448 K )
∴ V2 = 2.270 L
⇒ P2 = nRT2 / V2
⇒ P2 = (( 0.038 ) * ( 0.082 ) * ( 448 )) / 2.270
⇒ P2 = 0.615 atm * ( 760 mm Hg / atm ) = 467.37 mm Hg
Answer:
6 moles of oxygen, or 3O2.
Explanation:
I would build a proportion for this:
You can use P1V1/T1 = P2V2/T2 but since pressure is constant is becomes V1/T1=V2/T2
V1=0.5 L
T1=203 K
T2=273 K
V2=unknown
0.5L/203 = V2/273
V2= 0.67 L so C
Hope this helps :)
