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3 years ago

15

How to express as a chemical or condensed structural formula

1 answer:

Alisiya [41]3 years ago

4 0

I think it would be

Carbon + 2 Hydrogen= Carbon + Hydrogen + Carbon + 3 Hydrogen + 2 Bromine

But I’m not really sure, sorry if I’m wrong

Hope this helped

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Calculate the relative molecular mass of Ma(HCO3)2

Alex

Answer:I believe you mean Mg(HCO3)2. Since I have never heard of the element MA. but if you are calculating using mg(HCO3)2 your molar mass/ molecular mass will be 146.3387

Explanation:

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3 years ago

How many atoms are in 48.8 g of pure aluminum?

Alecsey [184]

there are 1023 atoms in pure aluminium

3 0

3 years ago

Which of the following is NOT a homogeneous mixture?

fenix001 [56]

Soy sauce?

sorry if it's wrong....

7 0

3 years ago

If 588 grams of FeS2 is allowed to react with 352 grams of O2 according to the following equation, how many grams of Fe2O3 are p

Rainbow [258]

<u>Answer:</u> The mass of iron (III) oxide produced is 782.5 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

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

<u>For </u> $FeS_2$ <u> :</u>

Given mass of $FeS_2$ = 588 g

Molar mass of $FeS_2$ = 120 g/mol

Putting values in equation 1, we get:

$\text{Moles of }FeS_2=\frac{588g}{120g/mol}=4.9mol$

<u>For </u> $O_2$ <u> :</u>

Given mass of $O_2$ = 352 g

Molar mass of $O_2$ = 32 g/mol

Putting values in equation 1, we get:

$\text{Moles of }O_2=\frac{352g}{32g/mol}=11mol$

The chemical equation for the reaction of $FeS_2$ and oxygen gas follows:

$FeS_2+O_2\rightarrow Fe_2O_3+SO_2$

By Stoichiometry of the reaction:

1 mole of $FeS_2$ reacts with 1 mole of oxygen gas

So, 4.9 moles of $FeS_2$ will react with = $\frac{1}{1}\times 4.9=4.9mol$ of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, $FeS_2$ is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of $FeS_2$ produces 1 mole of iron (III) oxide

So, 4.9 moles of $FeS_2$ will produce = $\frac{1}{1}\times 4.9=4.9moles$ of iron (III) oxide

Now, calculating the mass of iron (III) oxide from equation 1, we get:

Molar mass of iron (III) oxide = 159.7 g/mol

Moles of iron (III) oxide = 4.9 moles

Putting values in equation 1, we get:

$4.9mol=\frac{\text{Mass of iron (III) oxide}}{159.7g/mol}\\\\\text{Mass of iron (III) oxide}=(4.9mol\times 159.7g/mol)=782.5g$

Hence, the mass of iron (III) oxide produced is 782.5 grams

8 0

3 years ago

An atom has three full orbitals in its second energy level.

ICE Princess25 [194]

Orbitals am only hold two electrons each, so 3 orbitals can hold 6 electrons

7 0

3 years ago

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