Question

Help with 3.A and B image provided below​

Answer 1

a. P=0.971 atm=737.6 mmHg

b. n=2.88 x 10⁻³

Further explanation

Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

$\tt P_T=P_1+P_2+..P_n$

A. vapor pressure of water at 22.5 = 20.4 mmHg

Pt=P H₂ + P H₂O

758 = P H₂ + 20.4

P H₂=737.6 mmHg=0.971 atm

B.Ideal gas Law = PV=nRT

P = 0.971 atm

V = 72 ml = 0.072 L

R = 0.082 L/atm mol

T = 22.5 + 273.15 =295.65

$\tt n=\dfrac{0.971\times 0.072}{0.082\times 295.65}=2.88\times 10^{-3}$