1) The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the...

1) The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 87 ∘C ?

2) At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 70 ∘C ?

Expert Solution

Intilal Final

P1 = 2.1atm P2 =

T1 = 21C⁰ = 21+ 273 =294K T2 = 87C⁰ = 87 + 273 = 360K

P1/T1 = P2/T2

P2 = P1T2/T1

= 2.1*360/294 = 2.54atm

2. Intial Final

V1 = 22.4ml V2 =

T1 = 0C⁰ = 273 K T2 = 70C⁰ = 70 + 273 = 343K

V1/T1 = V2/T2

V2 = V1T2/T1

= 22.4*343/273 = 28.143L

queen_honey_blossom answered 1 year ago

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