Part 1 mass of H2 = 15.5g Molar mass of H2 = 2.01588g/mol No of mole of H2 = 15.
ID: 700303 • Letter: P
Question
Part 1
mass of H2 = 15.5g
Molar mass of H2 = 2.01588g/mol
No of mole of H2 = 15.5g/2.01588g/mol = 7.6889mole
Van der waals equation of state is
[P + a(n/V)2] [ (V/n) - b ] = RT
where,
P= pressure
a = constant , for H2 it is 0.2444L2atm/mol2
b = constant , for H2 it is 0.02661L/mol
V = volume , 1L
R = gas constant , 0.082057(L atm/mol K)
T = Temperature, 20 = 293.15K
Substituting the values
[ P + 0.2444(L2atm/mol2) (7.6889mol/1L)2][ (1L/7.6889mol) - 0.02661L/mol]= 0.082057(L atm/mol K ) × 293.15K
[ P + 1.8792atm][0.10344(L/mol)] = 24.055(L atm/mol)
[P+ 1.8792atm ] =232.55atm
P = 230.67atm
Part 2
Ideal gas equation is
PV = nRT
P = nRT/V
= 7.6889mol × 0.082057(L atm /mol K)×293.15K/1L
= 184.96atm
Explanation / Answer
CH 10 Required HW 12/19/17 14 Question (1 point) 2nd attempt Part 1 (0.5 point) Part 2 (0.5 point) 1st attempt