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
<span><span>NaOH + HCl --> NaCl + H2Oso here 1 mole of NaOH reacts with 1 mole of HCl. Hence it is required to convert the amount of HCl and NaOH in to moles.Number of HCl moles Concentration of the solution = 2.00M = 2 mol/ literVolume of the solution = 22.4 mlNumber of HCl moles = (2mol/1000 ml)*22.4 ml = 0.0448 mol</span></span>
The answer is True I hope this helps
True due to the fact that polymers are a giant chain of monomers