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Tems11 [23]
3 years ago
11

Combustion analysis of toluene, a common organic solvent, gives 3.52 mg of co2 and 0.822 mg of h2o. if the compound contains onl

y carbon and hydrogen, what is its empirical formula?
Chemistry
1 answer:
IRISSAK [1]3 years ago
7 0
<span>C7H8 First, lookup the atomic weight of all involved elements Atomic weight of carbon = 12.0107 Atomic weight of hydrogen = 1.00794 Atomic weight of oxygen = 15.999 Then calculate the molar masses of CO2 and H2O Molar mass CO2 = 12.0107 + 2 * 15.999 = 44.0087 g/mol Molar mass H2O = 2 * 1.00794 + 15.999 = 18.01488 g/mol Now calculate the number of moles of each product obtained Note: Not interested in the absolute number of moles, just the relative ratios. So not going to get pedantic about the masses involved being mg and converting them to grams. As long as I'm using the same magnitude units in the same places for the calculations, I'm OK. moles CO2 = 3.52 / 44.0087 = 0.079984 moles H2O = 0.822 / 18.01488 = 0.045629 Since each CO2 molecule has 1 carbon atom, I can use the same number for the relative moles of carbon. However, since each H2O molecule has 2 hydrogen atoms, I need to double that number to get the relative number of moles for hydrogen. moles C = 0.079984 moles H = 0.045629 * 2 = 0.091258 So we have a ratio of 0.079984 : 0.091258 for carbon and hydrogen. We need to convert that to a ratio of small integers. First divide both numbers by 0.079984 (selected since it's the smallest), getting 1: 1.140953 The 1 for carbon looks good. But the 1.140953 for hydrogen isn't close to an integer. So let's multiply the ratio by 1, 2, 3, 4, ..., etc and see what each new ratio looks like (Effectively seeing what 1, 2, 3, 4, etc carbons look like) 1 ( 1 : 1.140953) = 1 : 1.140953 2 ( 1 : 1.140953) = 2 : 2.281906 3 ( 1 : 1.140953) = 3 : 3.422859 4 ( 1 : 1.140953) = 4 : 4.563812 5 ( 1 : 1.140953) = 5 : 5.704765 6 ( 1 : 1.140953) = 6 : 6.845718 7 ( 1 : 1.140953) = 7 : 7.986671 8 ( 1 : 1.140953) = 8 : 9.127624 That 7.986671 in row 7 looks extremely close to 8. I doubt I'd get much closer unless I go to extremely high integers. So it looks like the empirical formula for toluene is C7H8</span>
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g Determine the empirical formula for a compound that contains C, H and O. It contains 40.92% C, 4.58% H, and 54.50% O by mass.
Lady bird [3.3K]

Answer:

The empirical formula for the compound is C3H4O3

Explanation:

The following data were obtained from the question:

Carbon (C) = 40.92%

Hydrogen (H) = 4.58%

Oxygen (O) = 54.50%

The empirical formula for the compound can be obtained as follow:

C = 40.92%

H = 4.58%

O = 54.50%

Divide by their molar mass

C = 40.92/12 = 3.41

H = 4.58/1 = 4.58

O = 54.50/16 = 3.41

Divide by the smallest i.e 3.41

C = 3.41/3.41 = 1

H = 4.58/3.41 = 1.3

O = 3.41/3.41 = 1

Multiply through by 3 to express in whole number

C = 1 x 3 = 3

H = 1.3 x 3 = 4

O = 1 x 3 = 3

The empirical formula for the compound is C3H4O3

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3 years ago
What are three ways to measure the amount of something chemistry?
AleksandrR [38]
There are three ways to measure the amount of something in chemistry.

1. There is a simple count which is tabulating the amount of something present. 

2. You can measure the mass which is the amount of matter in something. 

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Please comment the correct answer and I'll give you brainliest! Which atom of each pair below has the largest ionization energy?
monitta

Answer:kffffffffffffffffp;j.,,j,j[[;'/n  m

Explanation:

tggggggggggggggggggggggggggggggggggggggggggggggggggggggggggggg00000000000

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consider the phase change of ice to liquid water if the molar heat of fusion for water is 6.01 kj mol-1 how many joules are requ
uysha [10]

Answer:

The correct answer is 333.8 J

Explanation:

Ice (water in solid state) melts at 273 K (0ºC). During the phase change from solid to liquid, water absorbs 6.01 KJ per mol until it melts completely. To calculate the heat absorbed, we first have to convert the mass of water (1 g) to mol by using the molecular weight of water (H₂O):

Molecular weight of water= 2 x molar mass H + 1 x molar mass O

Molecular weight of water= 2 x 1 g/mol + 16 g/mol= 18 g/mol

mol ice= \frac{1 g}{18 g/mol}= 0.055 mol

heat= 0.055 mol x 6.01 KJ/mol= 0.3338 KJ

Finally, we convert KJ to J (1 KJ= 1000 J so we multiply by 1000):

0.3338 KJ x 1000 J/1 KJ= 333.8 J

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