According to Raoult's law, the partial pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the total pressure.

$p_1=x_1p_{total}$

where, x = mole fraction

$p_{total}$ = total pressure

$x_{oxygen}=\frac{\text {moles of oxygen}}{\text {total moles}}$ ,

$x_{oxygen}=\frac{3.0}{12.33}=0.243$ ,

$p_{oxygen}=0.243\times 770torr=187torr$

Thus the partial pressure of oxygen is 187 torr.

6 0

3 years ago

• 1. An object has a mass of 570g and a volume of 2280ml. Calculate its<br> density. 250 kg/m3

Dima020 [189]

Answer:

Density=mass/volume

= 570/2280

=0.25g/ml

7 0

3 years ago

Calculate the [H3O+] for orange juice, which has a [OH–] = 5.0 × 10–11 M.

zloy xaker [14]

Answer:

i Think.... i think its a carrot

Explanation: 5.0 x 10-11 M

3 0

3 years ago

Why is the theoritical strngth of metals much higher than that observed experimentally

fiasKO [112]

Not sure, but I would guess it's due to environmental factors, like heat, and imperfections in the metal. Just an educated guess, though.

5 0

3 years ago