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jenyasd209 [6]
2 years ago
5

1. How many moles are in 3.50 grams of NaCl?

Chemistry
1 answer:
Scrat [10]2 years ago
7 0
78 think that me the answer
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An organic liquid is a mixture of methyl alcohol (CH3OH) and ethyl alcohol (C2H5OH). A 0.220-g sample of the liquid is burned in
Artist 52 [7]

Answer:

Mass of Methyl alcohol (or methanol) = 0.1403g

Explanation:

<u>Step 1:</u> Given data

Mass of Sample: ms = 0.220 g

Mass of CO2: m0 = 0.345 g

Mass of CH3OH = m1

Mass of C2H5OH = m2

Molar mass CO2 = 44.01 g/mole

Molar mass CH3OH = 32 g/mole

Molar mass C2H5OH 46.07 g/mole

<u>Step 2: </u>Tjhe balanced equation

2 CH3OH + 3 O2 = 2 CO2 + 4 H2O

C2H5OH + 3 O2 =2 CO2 + 3 H2O

------------------------------------------------------

2 CH3OH + C2H5OH + 6 O2 = 4 CO2 + 7 H2O

<u>Step 3:</u> Calculate mass

In the balanced equation we notice that , the amount of CO2 is related to the amount of the alcohols: Moles CO2 = 4

mass of CO2 = Molar mass CO2((mass CH3OH/ Molar mass CH3OH)+(mass C2H5OH/Molar mass C2H5OH))

mass of CO2 = 44.01 ((mass CH3OH/ 32.04) + (mass C2H5OH/ 46.07)

The sample has a mass of 0.220 g = mass CH3OH + mass C2H5OH

mass C2H5OH = 0.220G - mass CH3OH

This we will insert in the equation, so we will only have 1 unknown mass

0.345g = 44.01((m1/32.04) + (2(0.220-m1)/M2) )

<=> m1 = ((mCO2/44.01)-(2*0.22/46.07))÷((1/32.04)-(2/46.07))

Thus: m1 = ((0.345/44.01)-(2*0.220/46.07))÷((1/32.04)-(2/46.07))

Thus m1 = 0.1403 g  = Mass of CH3OH

Since m2=(ms-m1).

m2 = 0.220-0.1403 = 0.0797 g = Mass of C2H5OH

Mass of methyl alcohol (Methanol) = 0.1403g

Mass of ethyl alcohol (Ethanol) = 0.0797g.

7 0
3 years ago
A sample of iodine is easiest to ship as a powder because it is making it easy to break into small pieces.What goes in the blank
Gemiola [76]
The answer is brittle 
7 0
3 years ago
Read 2 more answers
Please help!!
ludmilkaskok [199]

Answer:

yes, the law of conservation of mass hold true in this case burning magnesium strip is explained by this equation 2 Mg (s) + O2 (g) -> MgO (s)So the lighter magnesium, after reacting with oxygen in air, forms the heavier magnesium oxide. molar mass of magnesium and magnesium oxide are 24g and 40g respectively. So the same ratio 24:40 (i.e. 3:5) is maintained in the given masses of 48g and 80g, which means mass is conserved in the reacion.

Explanation:

Brainiest Please!!!

8 0
3 years ago
Read 2 more answers
If the vapor's volume were to be incorrectly recorded as 125ml, how will this error affect the calculated molar mass of the unkn
pishuonlain [190]
Since you didn't give the actual volume (or any of the experimental values) I can only tell you how to do it. Do the calculation using the real (determined) volume of the flask. Then, re-do the calculation with v = 125ml. Take the two values and calculate % error; m = measured vol; g = guessed vol. 

<span>[mW (m) - mW (g)]/mW (m) x 100% </span>

<span>(they want % error so, if it is negative, just get rid of the sign) </span>
3 0
3 years ago
What type of reaction is this?<br> 2 A1203 (s) + 4 Al(s) + 3 O2 (g)
GaryK [48]

Answer:

Decomposition

Explanation:

7 0
3 years ago
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