A 40.0 gram-sample of methanol, CH4O is mixed with 60.0 grams of ethanol, C2H6O. What is the mole fraction of the methanol?
1. A 40.0 gram-sample of methanol, CH4O is mixed with 60.0 grams of ethanol, C2H6O. What is the mole fraction of the methanol?
Given:
mass of solute = 40.0 g
mass of solvent = 60.0 g
solute: methanol (CH₄O)
solvent: ethanol (C₂H₆O)
Required:mole fraction of solute
Solution:Step 1: Calculate the molar mass of solute and solvent.
For solute
molar mass of solute = (12.01 g/mol × 1) + (1.008 g/mol × 4) + (16.00 g/mol × 1)
molar mass of solute = 32.042 g/mol
For solvent
molar mass of solvent = (12.01 g/mol × 2) + (1.008 g/mol × 6) + (16.00 g/mol × 1)
molar mass of solvent = 46.068 g/mol
Step 2: Calculate the number of moles of solute and solvent.
For solute
[tex]\text{moles of solute} = \frac{\text{mass of solute}}{\text{molar mass of solute}}[/tex]
[tex]\text{moles of solute} = \frac{\text{40.0 g}}{\text{32.042 g/mol}}[/tex]
moles of solute = 1.2483615 mol
For solvent
[tex]\text{moles of solvent} = \frac{\text{mass of solvent}}{\text{molar mass of solvent}}[/tex]
[tex]\text{moles of solvent} = \frac{\text{60.0 g}}{\text{46.068 g/mol}}[/tex]
moles of solvent = 1.3024225 mol
Step 3: Calculate the mole fraction of solute.
[tex]\text{mole fraction of solute} = \frac{\text{moles of solute}}{\text{moles of solute + moles of solvent}}[/tex]
[tex]\text{mole fraction of solute} = \frac{\text{1.2483615 mol}}{\text{1.2483615 mol + 1.3024225 mol}}[/tex]
[tex]\boxed{\text{mole fraction of solute} = 0.489}[/tex]
[tex]\\[/tex]
#CarryOnLearning
2. A solution contains 22.5 grams of methanol dissolved in sufficient water to give a total mass of 105.3 grams. The molar mass of methanol is 32.04 g/mol. What is the molality of the aqueous solution?
Strategy:
To calculate the molality of a solution, we need to know the number of moles of solute and the mass of the solvent in kilograms.
Solution:
The definition of molality (m) is
[tex]m = \frac{\text{moles of solute}}{\text{mass of solvent (kg)}}[/tex]
First, we find the number of moles of methanol in 42.2 g of methanol, using its molar mass as the conversion factor.
[tex]\text{moles of methanol} = \text{22.5 g methanol} \times \frac{\text{1 mol methanol}}{\text{32.04 g methanol}}[/tex]
[tex]\text{moles of methanol} = \text{0.70225 mol methanol}[/tex]
The mass of water is 105.3 g - 22.5 g = 82.8 g, or 0.0828 kg. Therefore,
[tex]m = \frac{\text{0.70225 mol methanol}}{\text{0.0828 kg H₂O}}[/tex]
[tex]\blue{m = 8.48 \: m}[/tex]
#CarryOnLearning
3. If 37g of methanol is produced from the reaction of 60 grams of co and 6 grams of h2, what is the limiting reagent
Answer:
akin na lng poin plsss tnx need ko po eh :-)
4. b. CALCULATE THE VOLUME OF 63.0 grams of liquid methanol if it's density is 0.791 g/ml?
SOLUTION:
Step 1: List the given values.
[tex]\begin{aligned} & m = \text{63.0 g} \\ & d = \text{0.791 g/mL} \end{aligned}[/tex]
Step 2: Calculate the density.
[tex]\begin{aligned} V & = \frac{m}{d} \\ & = \frac{\text{63.0 g}}{\text{0.791 g/mL}} \\ & = \boxed{\text{79.6 mL}} \end{aligned}[/tex]
Hence, the volume of methanol is 79.6 mL.
[tex]\\[/tex]
#CarryOnLearning
5. 2. A solution of methanol is prepared by dissolving 35.0 mL of methanol in water to give a total of 115.0 ml solution. What is the % by volume concentration of methanol?NONSENSE REPORT
Answer:30.43%
Explanation:
Weight. Weight of solute
%=------------------------------x100
Volume. Volume of solution
Hope it's help I'm grade 9
6. 5 examples of methanol
Answer:
kul4ng0t h3hi
ratatatat oh yeah ano ginagawa nyo ha
hoy masaya kaba
Explanation:
paints,varnishes,paint thinners, carburetor and various cleaning products
7. Calculate the volume of 63.0 grams of liquid methanol if its density is 0.791 g/ml?
Answer:
cywheyjkeb
Explanation:
ng ur fdguddm
8. Rubbing alcohol products sold in this pandemic contains methanol. A 1000 ml rubbing alcohol contains 7 ml of methanol. What is the percent by volume concentrration of methanol In the bottle
Answer:
7 persent
Explanation:
divide 7 by 1000
Answer:
A.1,000
sa na naka tolung
po
9. The density of methanol at 20oC is 0.791 g/mL. what is the mass in grams, of 250 mL sample?
SOLUTION:
Step 1: List the given values.
[tex]\begin{aligned} & d = \text{0.791 g/mL} \\ & V = \text{250 mL} \end{aligned}[/tex]
Step 2: Calculate the mass.
[tex]\begin{aligned} m & = dV \\ & = \text{(0.791 g/mL)(250 mL)} \\ & = \text{197.75 g} \\ & \approx \boxed{\text{198 g}} \end{aligned}[/tex]
Hence, the mass of the sample of methanol is 198 g.
[tex]\\[/tex]
#CarryOnLearning
10. The chemical formula of methanol is ch3oh. how many unshared electron pairs are associated with a molecule of methanol
https://brainly.ph/question/24385180?answering=true&answeringSource=feedPublic%2FhomePage%2F1
the chemical formula of methanol is CH3OH. How many unshared electrons pairs are associated with a molecule of methanol?
2
11. how many Carbon atoms does 100 grams of methanol contains?
Answer:
1 mol carbon-12 contains 6.022×1023 atoms. 1 mol H2O ... 1 mole of H2O molecules has a mass of 18.02 grams. molar mass in g/mol ...
12. A solution of methanol is prepared by dissolving 35 ml of methanol in water to give a total of 115 ml solution. what is the percent by volume concentration of methanol?
SOLUTION:
Step 1: List the given values.
[tex]\begin{aligned} & V_{\text{solute}} = \text{35 mL} \\ & V_{\text{solution}} = \text{115 mL} \end{aligned}[/tex]
Step 2: Calculate the percent by volume.
[tex]\begin{aligned} \%(v/v) & = \frac{V_{\text{solute}}}{V_{\text{solution}}} \times 100\% \\ & = \frac{\text{35 mL}}{\text{115 mL}} \times 100\% \\ & = 30.43478\% \\ & \approx \boxed{30.4\%} \end{aligned}[/tex]
Hence, the percent by volume concentration of methanol is 30.4%.
[tex]\\[/tex]
#CarryOnLearning
13. 3. A student obtains 100.0 g of methanol, CH3OH. How manymoles of methanol are present? How many methanolmolecules are present?
Solution (Moles of Methanol):
Step 1: Calculate the molar mass of methanol (CH₃OH).
molar mass = (12.01 g/mol × 1) + (1.008 g/mol × 4) + (16.00 g/mol × 1)
molar mass = 32.042 g/mol
Step 2: Calculate the number of moles of methanol.
[tex]\text{moles of CH₃OH = 100.0 g CH₃OH} × \frac{\text{1 mol CH₃OH}}{\text{32.042 g CH₃OH}}[/tex]
[tex]\boxed{\text{moles of CH₃OH = 3.121 mol}}[/tex]
Solution (Number of Methanol Molecules):
[tex]\text{number of CH₃OH molecules = 100.0 g CH₃OH} × \frac{\text{1 mol CH₃OH}}{\text{32.042 g CH₃OH}} × \frac{\text{6.022 × 10²³ CH₃OH molecules}}{\text{1 mol CH₃OH}}[/tex]
[tex]\boxed{\text{number of CH₃OH molecules = 1.8794 × 10²⁴ molecules}}[/tex]
#CarryOnLearning
14. III. 100 grams of HCl reacts with 96 grams of methanol CH3OH, producing chloromethane, CH3Cl and water according to the following equation:CH3OH + HCI CH3Cl + H20 a. What is the limiting reagent? b. How many grams of CH CI will be produced? c. If 76 grams of CH3Cl is actually produced, what is the percent yield?
Answer:
I hope this helps!!
#CarryOnLearning
#RoadToGenius
15. Methanol types of drink
Answer:
Methanol (CH3OH), also called methyl alcohol, wood alcohol, or wood spirit, the simplest of a long series of organic compounds called alcohols, consisting of a methyl group (CH3) linked with a hydroxy group (OH). Methanol was formerly produced by the destructive distillation of wood.
16. characteristics of the methanol
1Physical Description. Methanol appears as a colorless fairly volatile liquid with a faintly sweet pungent odor like that of ethyl alcohol. Completely mixes with water. The vapors are slightly heavier than air and may travel some distance to a source of ignition and flash back.
Explanation:
colorless liquid with pungent odor
17. Effects of methanol in human
methanol causes poisoning in human body
18. 13. Why is it dangerous for man to take in methanol?a. Methanol, when taken in causes lead poisoning.b. Methanol, when oxidized, turns into ethanol.c. Methanol, when oxidized, produces formaldehyde and formic acidwhich are highly toxic to the cells.d. Methanol, when oxidized forms carbon.
Answer:
I think its (C.)
but im not sure if im correct
Answer:
C.po
Explanation:
kung mali po paki sabi.
salamat
19. How Many Grams Of Methanol Are Contained In 0.100 L Of 1.7 M Aqueous Ethanol?
Answer:
5.48 g
Explanation:
M = n/V
1.71 = n/0.100
n = 0.171 mol
The molar mass of methanol is 32.04 g/mol, and it is the mass (m) divided by the number of moles:
FM = m/n
32.04 = m/0.171
m = 5.48 g
Sana maka tulong :)
20. what is methanol? nonpolar or polar?
Explanation:
Methanol: a nondrinking type of alcohol which is mostly used to create fuel, solvent and antifreeze.
Nonpolar: a nonpolar molecule has no separation of charge, so no positive or negative poles are formed. In other words, the electrical charges fof nonpolar molecules are evenly distributed across the molecule.
Polar: Polar molecules occur when there is an electronegativity difference between the bonded atoms.
21. 1.Dissolve 15 grams of sugar in 150 grams of solution.Compute for the concentration by mass.2.Determine the percent by volume of solution made by combining 20 ml of methanol with enough water to produce 180 ml of the solution.
d ko alm
Explanation:
sorry po
btw thanks sa points
22. 42g of methanol is dissolved in 800g of water. Calculate the percentage of methanol solution?
Answer:
4.99%
Explanation:
I'm not sure, correct me if I'm wrong
23. (3 points) Suppose methanol will be burned in air. If 209 grams of this substance are used up in the reaction, how many grams of water are produced?
Methanol burns as,
CH₃OH + 3/2 O₂ → CO₂ + 2 H₂O.
But assumption on stoichiometric coefficients does not hold for mass. We need to convert it to moles.
Molar mass of CH₃OH = 12+(4×1)+16 = 32
Moles of CH₃OH given = 209/32 = 6.53 mol.
1 mol CH₃OH ⇒2 mol H₂O
6.53 mol CH₃OH ⇒(2×6.53) mol H₂O
13.06mol H₂O = 13.06 × 18 g H₂O = 235.08 g.
24. Calculate the mole fraction of c2h5oh in a solution that contains 46 grams of ethanol, c2h5oh, and 64 grams of methanol, ch3oh
SOLUTION:
Step 1: List the given values.
[tex]\begin{aligned} & mass_{\text{ethanol}} = \text{46 g} \\ & MM_{\text{ethanol}} = \text{46.069 g/mol} \\ & mass_{\text{methanol}} = \text{64 g} \\ & MM_{\text{methanol}} = \text{32.042 g/mol} \end{aligned}[/tex]
Step 2: Calculate the number of moles of ethanol and methanol.
• For ethanol
[tex]\begin{aligned} n_{\text{ethanol}} & = \frac{mass_{\text{ethanol}}}{MM_{\text{ethanol}}} \\ & = \frac{\text{46 g}}{\text{46.069 g/mol}} \\ & = \text{0.9985 mol} \end{aligned}[/tex]
• For methanol
[tex]\begin{aligned} n_{\text{methanol}} & = \frac{mass_{\text{methanol}}}{MM_{\text{methanol}}} \\ & = \frac{\text{64 g}}{\text{32.042 g/mol}} \\ & = \text{1.9974 mol} \end{aligned}[/tex]
Step 3: Calculate the mole fraction of ethanol
[tex]\begin{aligned} X_{\text{ethanol}} & = \frac{n_{\text{ethanol}}}{n_{\text{methanol}} + n_{\text{ethanol}}} \\ & = \frac{\text{0.9985 mol}}{\text{1.9974 mol + 0.9985 mol}} \\ & = \boxed{0.333} \end{aligned}[/tex]
Hence, the mole fraction of ethanol is 0.333.
[tex]\\[/tex]
#CarryOnLearning
25. what is the percent by volume of methanol solution if it contains 22.60mL methanol and 58.36mL of water? with solution.
Answer:
27.92%
Explanation:
26. 25 ml of methanol is mixed with 150ml of water. what is the volume of methanol
25 ml of methanol is mixed with 150ml of water. what is the volume of methanol
Answer:
16.67 %
Explanation:
27. 1.denatured alcohol contains 90% ethanol and 10% methanol which is the solute and which is the solvent in the solution?a.solute-ethanol, solvent-methanolb.solute-ethanol, solvent-water c.solute-methanol, solvent-ethanol d.solute-methanol,solvent-water
Answer:
c
Explanation:
ethanol is a solvent because it has a greater amount while methanol is a solute because it has a less amount
28. what is the percent by volume of methanol in a 90ml solution that contains 25ml methanol?
Answer:
27.8%
Explanation:
I guess that is right
Answer:
So, you have 90 mls of total solution, and of that, 25 mls is isopropanol. The % by volume = 25 ml/90 ml (x100%) = 27.8% by volume.
Explanation:
#CarryOnLearning
#Brainliest
29. A solution of methanol is prepared by dissolving 35.0 mL of methanol in water to give a total of 115.0 mL solution. What is the % by volume concentration of methanol? PA HELP NAMAN PO THANKS!
[tex]Hence \: the \: answer \: is, 30.4(percent)[/tex]
[tex]Please \: see \: the \: pic \: that \: I \: attached, \: you \: can \: see \: the \: solution...[/tex]
30. The density of methanol at 20°C is 0.791 g/mL. What is the mass, in grams of a 280 mL sample?
Answer:
221.48 g(rams).
Step-by-step explanation:
In this given case of density, for every milliliter, we have 0.791 grams. Let's just multiply the grams by 280 then.
[tex]0.791 \times 280 = 221.48[/tex]
