Question

If 15.82 mol of helium gas is at 12.4 ∘C and a gauge pressure of 0.339 atm .

Part A: Calculate the volume of the helium gas under these conditions.

Part B: Calculate the temperature if the gas is compressed to precisely half the volume at a gauge pressure of 1.19 atm.

Answer 1

SOLUTION:

n= 15.82 mol

R= 8.31 J/mol.K

P= 0.339 atm= 0.339*101325 pa= 34349.18 pa

T= 12.4+273.15 K= 285.55 k

A) we know that, for ideal gas formula

PV= nRT

V= 1.093 m^{​​​​​​3}

The volume of helium is = 1.093 m^{​​​​​​3}

B) P^{​​​​​​'} = 1.19*101325 pa

V^{​​​​​​'} = 1.093/2 m^{​​​​​​3}

Then the temperature is = T

Applying this formula

P^'V^{​​​​'} = nRT

(1.19*101325)(1.093/2)=15.82(8.31)T

T= 501.24 K

The temperature is