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3 years ago

Write the empirical formula of at least four binary ionic compounds that could be formed from the following ions:

Chemistry

2 answers:

Tema [17]3 years ago

8 0

Answer:

MgI₂

MgO

PbI₄

PbO₂

Explanation:

Binary compounds are formed when a cation combines with an anion. Such compounds are also known as ionic compounds.

The four binary compounds that can be formed are as follows:

Mg²⁺ I⁻

When writing the empirical formula the charge of the anion is written as the subscript of the cation, and the charge of the cation is written as the as script of the anion, such as

Mg₁I₂ or MgI₂

Mg²⁺ O²⁻

Mg₂O₂ or MgO

Pb⁴⁺ I⁻

Pb₁I₄ or PbI₄

Pb⁴⁺ O²⁻

Pb₂O₄ or PbO₂

cupoosta [38]3 years ago

4 0

MgO
MgI2
PbO2
PbI4

These are the possible compounds

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Volume* density=MASS

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Which of the following elements has a complete outer shell of electrons? A. Iron (Fe) B. Hydrogen (H) C. Neon (Ne) D. Nitrogen (

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Answer:

The answer is Neon

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3 years ago

If the mass percentage composition of a compound is 72.1% Mn and 27.9% O, its empirical formula is

mojhsa [17]

Answer:

MnO- Manganese Oxide

Explanation:

Empirical formula: This is the formula that shows the ratio of elements

present in a

compound.

How to determine Empirical formula

1. First arrange the symbols of the elements present in the compound

alphabetically to determine the real empirical formula. Although, there

are exceptions to this rule, E.g H2So4

2. Divide the percentage composition by the mass number.

3. Then divide through by the smallest number.

4. The resulting answer is the ratio attached to the elements present in

a compound.

Mn O

% composition 72.1 27.9

Divide by mass number 54.94 16

1.31 1.74

Divide by the smallest number 1.31 1.31

1 1.3

The resulting ratio is 1:1

Hence the Empirical formula is MnO, Manganese oxide

8 0

3 years ago

112 g of aluminum carbide react with 174 g water to produce methane and aluminum hydroxide in the reaction shown below.

dolphi86 [110]

<u>Answer:</u> 4.999 moles of excess reactant will be left over.

<u>Explanation:</u>

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of aluminium carbide = 112 g

Molar mass of aluminium carbide = 143.96 g/mol

Putting values in equation 1:

$\text{Moles of aluminium carbide}=\frac{112g}{143.96g/mol}=0.778mol$

For the given chemical reaction:

$2Al_4C_3(s)+12H_2O(l)\rightarrow 3CH_4(g)+4Al(OH)_3(s)$

By the stoichiometry of the reaction:

2 moles of aluminium carbide reacts with 12 moles of water

So, 0.778 moles of aluminium carbide will react with = $\frac{12}{2}\times 0.778=4.668 mol$ of water

Given mass of water = 174 g

Molar mass of water = 18 g/mol

Putting values in equation 1:

$\text{Moles of water}=\frac{174g}{18g/mol}=9.667mol$

Moles of excess reactant (water) left = 9.667 - 4.668 = 4.999 moles

Hence, 4.999 moles of excess reactant will be left over.

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2 years ago

Which best describes the motion of molecules in the gaseous state?

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Answer:

They spread apart to fill the enclosed object. In other words they move freely...

hope this helped you

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3 years ago