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pickupchik [31]
3 years ago
15

An organic compound is composed of 38.7% C, 9.70% H, 51.6% O. The compound has a molecular formula mass of 62.0g/mol.

Chemistry
2 answers:
Tcecarenko [31]3 years ago
5 0

<span>B)<span>C2H6O<span>2
</span></span></span>
First, convert each percentage to grams: 38.7g, 9.70g, and 51.6g. 
Next, calculate the number of moles of each element, based on the number of grams given.
C = 3.23 mol
H = 8.91 mol
O = 3.23 mol
Set up the ratio of moles of each element:
C3.34H9.70O3.23. Convert the decimals to whole numbers by dividing by the smallest subscript, 3.23.
The empirical formula is CH3O.
Now, compute the formula mass, which is 31. Finally, divide the molecular mass by the formula mass, 62/31 = 2. Multiple the subscripts by 2 to get the molecular formula.
katovenus [111]3 years ago
5 0

Answer:

B) C_{2}H_{6}O_{2}

Explanation:

First you should add up the three percentages:

38.7+9.70+51.6 = 100

Then you take that base of 100g to calculate the mass of each element:

C=38.7g

H=9.70g

O=51.6g

Then you find the number of moles of each element using the molar mass of each one:

- For C:

38.7gC*\frac{1molC}{12gC}=3.22molesC

- For H:

9.70gH*\frac{1molH}{1gH}=9.70molesH

- For O:

51.6gO*\frac{1molO}{16gO}=3.22molesO

Then, you find the minimum number of moles and divide each one by it:

- For C:

\frac{3.22}{3.22}=1

- For H:

\frac{9.70}{3.22}=3

- For O:

\frac{3.22}{3.22}=1

You have find the proportion of each element in the compound that is CH_{3}O, but you should find the molecular formula taking in account the molar mass of the compound, so:

(2.molarmassC)+(6.molarmassH)+(2.molarmassO)=62.0\frac{g}{mol}

(2*12\frac{g}{mol})+(6*1\frac{g}{mol})+(2*16\frac{g}{mol})=62.0\frac{g}{mol}

So the molecular formula is C_{2}H_{6}O_{2}

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Zielflug [23.3K]

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Anode(+): 2Cl^-\rightarrow Cl_2+2e^-

b) 0.640 grams of Ba will be deposited.

Explanation:  a) The problem is based on Faraday law of electrolysis. Molten barium chloride has Ba^+^2 ion and Cl^- ion. Barium ion is reduced and chloride is oxidized. Reduction takes place at cathode and oxidation at anode. So, the half reactions will be:

Cathode(-): Ba^+^2+2e^-\rightarrow Ba

Anode(+): 2Cl^-\rightarrow Cl_2+2e^-

b) The question asks, how many grams of barium metal can be produced by supplying 0.50 ampere for 30 minutes.

From the Cathode half-reaction, 1 mole of Ba is deposited by 2 moles of electrons and we know that 1 mole of electron carries one Faraday that is 96485 Coulomb.

Coulombs for 2 moles of electrons will be = 2*96485 C = 192970 C

So, we can say that, 192970 C will deposit 1 mole of Ba metal.

Total available coulombs can be calculated using the formula:

q=i*t

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q=q=0.50A*30min(\frac{60sec}{1min})

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Let's calculate how many moles of Ba will get deposited by 900 C.

900C(\frac{1molBa}{192970C})

= 0.00466 mole Ba

Convert the moles of Ba to grams and for this we multiply by molar mass of Ba which is 137.33 gram per mol.

0.00466molBa(\frac{137.33g}{1mol})

= 0.640 g Ba

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a prescriber has ordered childrens motrin 400 mg po q6h for a child who weighs 60 kg. how many mg/kg is the child receiving
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5 0
1 year ago
A certain metal M forms a soluble sulfate salt MSO, Suppose the left half cell of a galvanic cell apparatus is filled with a 3.0
bija089 [108]

Answer:

E = 0.062 V

Explanation:

(a) See the attached file for the answer

(b)

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Substituting, we have

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5 0
2 years ago
How much heat is required to change 100 g of ice (H2O) at 253 K to vapor (steam) at 393 K?
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<u>Explanation: </u>

To calculate the amount of heat required, we use the formula:

Q= m\times c\times \Delta T

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Putting values in above equation, we get:

\Delta T={\text{Change in temperature}}=(393-253)K=140K=140^oC

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Thus, heat released by 100 grams of ice is 58.604kJ.

3 0
3 years ago
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