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3 years ago

How many moles of CO2 are produced when 1 mole wax C31H64 is burned? 31 32 64 or 47

Chemistry

2 answers:

IRISSAK [1]3 years ago

5 0

Answer:

31 moles.

Explanation:

The products of combustion are CO2 and H2O.

C31H64 + 47O2 ---> 31CO2 + 32H2O

Lana71 [14]3 years ago

4 0

Answer:

31 moles

Explanation:

The balanced combustion reaction of the wax, $C_{31}H_{64}$ is shown below as:

$C_{31}H_{64}+47O_2\rightarrow 31CO_2+32H_2O$

As seen from the reaction,

1 mole of wax, $C_{31}H_{64}$ on combustion produces 31 moles of carbon dioxide, $CO_2$

Hence, moles of $CO_2$ when 1 mole of wax, $C_{31}H_{64}$ is burnt = 31 moles

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3 years ago

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Calculate the molar mass of aspirin, C9H8O4

Vladimir79 [104]

Add up all the molar masses of the elements multiplied by the number of atoms each.

Molar mass of carbon = 12.01g
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4 years ago

Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. if 4.40 mol of m

Georgia [21]

The balanced chemical equation for the above reaction is as follows ;
Mg + 2HCl —> MgCl2 + H2
The stoichiometry of Mg to HCl is 1:2
This means that 1 mol of Mg reacts with 2 mol of HCl
Equal amounts of both Mg and HCl have been added. One reagent is the limiting reactant and other reactant is in excess.
Limiting reactant is the reagent that is fully used up in the reaction and the amount of Product formed depends on the amount of limiting reactant present.
In this reaction if Mg is the limiting reactant, 4.40 moles of Mg should react with 4.40x2 -8.80 moles of HCl.
But only 4.40 moles of HCl present therefore HCl is the limiting reactant that reacts with 4.40/2 = 2.20 moles of Mg
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4 years ago

A sample of an unknown metal has a mass of 22.4g. A graduated cylinder contains 3.2 ml of water. After the metal sample is added

Goshia [24]

Answer:

d = 14.9 g/mL

Explanation:

Given data:

Mass of metal = 22.4 g

Volume of eater = 3.2 mL

Volume of water + metal = 4.7 mL

Density of metal = ?

Solution:

Volume of metal:

Volume of metal = volume of water+ metal - volume of water

Volume of metal = 4.7 mL - 3.2 mL

Volume of metal = 1.5 mL

Density of metal:

d = m/v

d = density

m = mass

v = volume

d = 22.4 g/ 1.5 mL

d = 14.9 g/mL

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3 years ago

(a) calculate the %ic of the interatomic bond for the intermetallic compound tial3. (b) on the basis of this result, what type o

Mrrafil [7]

Answer :

The correct answer is %IC = 10 % and bond is covalent bond with slight polarity.

Percent Ionic Character :

It is defined as percent of ionic character present in a polar covalent bond . The formula of % ionic character (%IC) is given as follows :

$Percent Ionic character = 1 - e^-^0^.^2^5 ^*^(^X^a^-^X^b^) * 100$

Where Xa = Electronegativity of A atom and Xb = Electronegativity of B atom

Given : Molecule is TiAl₃

Electronegativity of Ti = 2.0

Electronegativity of Al = 1.6 ( From image shared )

Plug the value in above formula :

$Percent Ionic character = 1 - e^-^0^.^2^5 ^*^(^2^.^0^-^1^.^6^) * 100$

$Percent Ionic character = 1 - e^(^-^0^.^2^5 ^*^0^.^4^) * 100$

$Percent Ionic character = 1 - e^(^-^0^.^1^) * 100$

Value of e⁻¹ = 0.90

Percent ionic character = 1 - 0.90 * 100

Percent Ionic character = 10 %

Since the % IC is 10 % , which is very less comparatively , hence the bond is covalent and very less polar .

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3 years ago