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yaroslaw [1]
3 years ago
10

You perform a combustion analysis on a 255 mg sample of a substance that contains only C, H, and O, and you find that 561 mg of

CO2 is produced, along with 306 mm of H2O.
if the substance contains only C, H, and O, what is the empirical formula
if the molar mass of the compound is 180 g/mol what is the molecular formula of the compound
Chemistry
2 answers:
alexgriva [62]3 years ago
6 0

Answer:

molecular formula of compound =C₉H₂₄O₃

Explanation:

The compound contains only C,H and O

The combustion equation for carbon is:

C+O_{2}-->CO_{2}

Thus if we are obtaining 44g of carbon dioxide it means the amount of carbon is 12g.

If we are getting 1g of carbon dioxide, it means the amount of carbon = \frac{12}{44}g

If we are getting 561mg of carbon dioxide, it means the amount of carbon=\frac{12X561}{44}=153mg

So the mass of carbon in the given sample = 153mg

Percentage of carbon = \frac{massofcarbonX100}{massofsample}=\frac{153X100}{255}=60

The combustion equation for hydrogen is:

H_{2}+0.5O_{2}-->H_{2}O

Thus if we are obtaining 18g of water it means the amount of hydrogen is 2g.

If we are getting 1g of water, it means the amount of hydrogen = \frac{2}{18}g

If we are getting 306mg of water, it means the amount of hydrogen=\frac{2X306}{18}=34mg

So the mass of hydrogen in the given sample = 34mg

Percentage of hydrogen = \frac{massofhydrogenX100}{massofsample}=\frac{34X100}{255}=13.33

Percentage of oxygen=100-(60+13.33)=26.67%

The moles of each element in 100g of sample will be

moles of carbon = \frac{mass}{atomicmass}=\frac{60}{12}=5

moles of hydrogen = \frac{mass}{atomicmass}=\frac{13.33}{1}=13.33

moles of oxygen = \frac{mass}{atomicmass}=\frac{26.67}{16}=1.67

Let us divide all the moles with 1.67

moles of carbon = 3

moles of hydrogen = 8

moles of oxygen = 1

So the empirical formula of the compound would be:C₃H₈O

The empirical mass = 60

molar mass = 180g

So the molecular formula will be = \frac{180}{60}Xempiricalformula

molecular formula=C₉H₂₄O₃

zhuklara [117]3 years ago
5 0
The combustion of an organic compound is mostly written as,
                        CaHbOc + O2 --> CO2 + H2O
where a, b, and c are supposed to be the subscripts of the elements C, H, and O in the compound. Determining the number of moles of C and H in the product which is the same as that in the compound,
   (Carbon, C)   :   (561 mg) x (12/44) = 153 mg x (1 mmole/12 mg) = 12.75
   (Hydrogen, H) :  (306 mg) x (2/18)  = 34 mg x (1 mmole/1 mg) = 34 
   Calculating for amount of O in the sample,
(oxygen, O) = 255 - 153 mg - 34 mg = 68 mg x (1mmole/16 mg) = 4.25 
The empirical formula is therefore,
                        C(51/4)H34O17/4
                           C3H8O1
The molar mass of the empirical formula is 60. Therefore, the molecular formula of the compound is,
                                C9H24O3
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Answer:

The reaction will occur, in the forward direction, and NiO will be reduced to Ni

Explanation:

Step 1: Data given

Kp = 6.0 * 10²

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Step 2: The balanced equation:

NiO(s) + CO(g) ⇆ Ni(s) + CO2(g)

Step 3: Calculate P(CO) and P(CO2)

For this equilibrium, the expression for Kp is:

Kp = P(CO2)/P(CO) = 6.0*10^2

(NiO and Ni are solids so do not change anything to the Kp

⇒ with P(CO) = 150 torr

⇒ P(CO) = 760 - 150 = 610 torr

Step 4: Calculate the reaction quotient

Q = 610/150 = 4.1

Q<<< Kp

There are more reactants than products. As a result, some of the reactants will become products, causing the reaction to shift to the right.

This means the reaction will proceed in the forward direction, and NiO will be reduced to Ni.

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Use the following equation to answer the questions below:
Gala2k [10]

Explanation:

The equation of the reaction is given as;

Be + 2HCl → BeCl2 + H2

What is the mass of beryllium required to produce 25.0g of beryllium chloride?

1 mol of Be produces 1 mol of BeCl2

Converting to mass;

Mass = Molar mass  *  Number of moles

9.01g of Be produces 79.92g of BeCl2

xg of Be produces 25g of BeCl2

Solving for x;

x = 25 * 9.01 / 79.92

x = 2.82 g

What is the mass of hydrochloric acid required to produce 25.0g of beryllium chloride? g

Converting 25.0g of beryllium chloride to moles;

Number of moles = Mass / Molar mass

Number of moles = 25 / 79.92 = 0.3128 mol

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x mol of HCl would produce 0.3128 mol of BeCl2

solving for x;

x = 0.3128 * 2 = 0.6256 mol

Converting to mass;

Mass = 0.6256 * 36.5 = 22.83 g

What is the mass of hydrogen gas produced when 25.0g of beryllium chloride is also produced? g

25g of BeCl2 = 0.3128 mol of BeCl2

From the equation;

1 mol of H2 is produced alongside 1 mol of BeCl2

This means;

0.3128 mol of H2 would also be produced alongside 0.3128 mol of BeCl2

Mass = Number of moles * Molar mass

Mass = 0.3128mol * 2.0159 g/mol = 0.6306 g

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Bingel [31]

Answer:

Explanation:

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