Answer:
16.5 atm
Explanation:
<em>A mixture of He, N₂, and Ar has a pressure of 24.1 atm at 28.0 °C. If the partial pressure of He is 3013 torr and that of Ar is 2737 mm Hg, what is the partial pressure of N₂?</em>
The total pressure of a gaseous mixture is equal to the sum of the partial pressures.
P = pHe + pN₂ + pAr
pN₂ = P - pHe - pAr [1]
We need to express pHe and pAr in atm.
From [1],
pN₂ = 24.1 atm - 3.96 atm - 3.60 atm = 16.5 atm
Answer:
sorry this is a kind of confusing question.
Explanation:
The name is Copper(II) Oxide and/or Cupric Oxide.
Cu is Copper and O is Oxygen.
Usually when the Oxygen ion is placed after another, it's name is Oxide.
Answer:
The empirical formula is the simplest form;
Given:
Oxygen O at 94.1% and
H at 5.9%
Assume 100grams.
94% = 0.941 x 100gm. = 94.1 gm x 1mole/16gm. = 5.88 moles of O
5.9% = 0.059 x 100gm. = 5.9gm. X 1moleH/1.002gm. = 5.88 moles of H
There is one mole of O for each mole of H so the empirical formula is 
and written as OH.
The empirical formula for 200 grams of an organic sample which contains carbon,hydrogen, and oxygen is C3H6O
