Answer:
a) 742.1 mm Hg O2
b) 0.4434 g O2
c) 0.01386 mol O2
Explanation:
<u>Step 1:</u> Data given
Mass of the sample = 3.6349 grams
volume of oxygen = 346.2 mL
Temperature = 23.6 °C
atmospheric pressure = 763.4 mmHg
<em><u>Step 2:</u></em><em> </em><em>What is the partial pressure of the oxygen? </em>
<em><u /></em>
763.4 mmHg - 21.3 mmHg = 742.1 mm Hg O2
<em>b. What mass of oxygen was liberated?</em>
All of the mass lost by the reactants was due to oxygen being liberated.
(3.6349 g) - ( 3.1915 g) = 0.4434 g O2
<em>c. How many moles of oxygen were produced?</em>
(0.4434 g O2) / (32 g O2/mol) = 0.01386 mol O2
Answer:
Explanation:
At high elevations the atmospheric pressure is lower. That means that slower moving molecules of water at the surface meet with less resistance from the atmospheric pressure. So the water begins to escape with less energy needed. The boiling point goes from 100 at sea level to about 93 degrees about 6000 feet up.
Answer: acetic acid structure
Explanation:
In the lewis structure we have 24 valence electrons