Question

at 120.0 c the pressure of a sample of nitrogen is 1.07 atm. what will the pressure be at 205 c assuming constant volume?

Answer 1

1.30 atm (rounded)

Step-by-step explanation:

P1= 1.07 atm

P2= ?

T1= 122 Celsius (+273 to convert to Kelvin)= 395 K

T2= 205 Celsius (+273 to convert to Kelvin)= 478 K

`(P1)/(T1) = (P2)/(T2)`

`(1.07 atm)/(395 K) =(P2)/(478 K)`

`P2=((1.07 atm) (478 K))/(395 K)`

`=(511.46)/(395) = 1.29483544304`

= 1.30 atm

Answer 2

We can use the ideal gas equation which is expressed as PV = nRT. At a constant volume and number of moles of the gas the ratio of T and P is equal to some constant. At another set of condition, the constant is still the same. Calculations are as follows:

T1/P1 = T2/P2

P2 = T2 x P1 / T1

P2 = 393.15 K x 1.04 atm / 478.15 K

P2 = 0.86 atm