6.81% is the percent yield when 12 g of CO2 are formed experimentally from the reaction of 0.5 moles of C8H18 reacting with excess oxygen.
Explanation:
Data given:
mass of carbon dioxide formed = 12 grams (actual yield)
atomic mass of CO2 = 44.01 grams/mole
moles of 
= 0.5
Balanced chemical reaction:
2 + 25 
⇒ 16 C + 18 
number of moles of carbon dioxide given is
number of moles = 
number of moles= 
number of moles of carbon dioxide gas = 0.27 moles
from the reaction 2 moles of reacts to produce 16 moles of C
So, when 0.5 moles reacted it produces x moles
= 
x = 4
4 moles of carbon dioxide formed, mass from it will give theoretical yield.
mass = number of moles x molar mass
mass = 4 x 44.01
= 176.04 grams
percent yield =
x 100
percent yield = 
x 100
percent yield = 6.81 %
Answer: It's all in the screenshot
Explanation: Got it right on edg
<span> E = h v where v = frequency h = plancks constant 6.626 * 10 - 34
4.8 * 6.626 = 31.8 </span>
Answer:Step 1: Gather the Needed Materials (coffee Filter, Pencil, Beaker, Water Soluble Pen/marker, Water) Step 2: Cut a Strip of Filter Paper From the Coffee Filter and Using the Marker Draw a Thick Line Near the Bottom of the Filter Paper- About 1/4 Inch From the Bottom. Step 3: Allow the Water to Move Up the Paper for Approx. 5 Minutes and Then Remove the Strip From the Water Step 4: Students Should Identify the Individual Colors in the Chromatogram That Make Up the Markers Unique Mix of Ink. Step 5: Once Students Have Mastered the Technique Its Time to Put Their Skills to the Test in "The Case of the Celebrity Dog-napping" Step 7: Write the Ransom Note on a Piece of Filter Paper in One of the Suspect Inks.
Explanation: Chromatography is the physical separation of a mixture into its individual components. This lesson integrates mixtures, solutions & solubility into an activity where students will identify the solute & the solvent. Because chromatography can be used to separate the components of inks & dyes, students are able to identify the unique "recipe" that makes up the mixture of a specific brand of pen. After the students are taught the ink chromatography technique, the fun can continue with a mini forensic investigation, "The Case of the Celebrity Dog-napping".
hopes this helps
Answer:
The moles of KClO3 = 0.052 moles
Explanation:
Step 1: Calculate the pressure of oxygen gas
The oxygen has a total pressure (including water vapour) of 760 mmHg
The pressure of Oxygen = (760 - 26) mmHg
= 734 mmHg of water vapor
Step 2: Calculate the no of moles of oxygen
Using Ideal gas equation
P V = n R T
P = pressure of oxygen in N/m2 ( you should convert 734 mmHg to pascal or N/m2) = 97,858.6 N/m2 or pas
V = 2 litres = 0.002 m3
R = gas constant = 8.31
T= 27oC = 300 K
Applying this equation P V = n R T
97,858.6 x 0.002 = n x 8.31 x 300
n = 0.0785 mol of Oxygen
From the balanced equation
2 KClO 3 ---- 2 KCl + 3 O 2
3 moles of oxygen is produced from 2 moles KClO3
so 0.0785 mole of oxygen will be produced from x
x = (0.0785 x 2 ) / 3
x = 0.052 moles of KClO3
