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3 years ago

2N2 + O2 -------> 2 N2O

Chemistry

1 answer:

notka56 [123]3 years ago

8 0

Answer:

Explanation:

Given data:

Mass of N₂ = 48.7 g

Moles of N₂ = ?

Molecules of N₂ = ?

Mass of N₂O = ?

Moles of N₂O = ?

Atoms of N₂O = ?

Solution:

Chemical equation:

2N₂ + O₂ → 2N₂O

Number of moles of N₂:

Number of moles = mass/ molar mass

Number of moles = 48.7 g / 28 g/mol

Number of moles = 1.74 mol

Number of molecules of N₂:

1 mole = 6.022 × 10²³ molecules

1.74 mol× 6.022 × 10²³ molecules/1 mol

10.5 × 10²³ molecules

Now we will compare the moles of N₂ with N₂O from balance chemical equation:

N₂ : N₂O

2 : 2

1.74 : 1.74

Moles of N₂O:

1.74 mol

Mass of N₂O:

Mass = number of moles × molar mass

Mass = 1.74 mol × 44 g/mol

Mass = 76.56 g

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Mars2501 [29]

C: 0.012 mol.

<h3>Explanation</h3>

Start with 0.0020 moles of iodate ions ${\text{IO}_{3}}^{-}$ .

How many moles of iodine $\text{I}_2$ will be produced?

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$\text{I}_2$ reacts with ${\text{S}_2\text{O}_3}^{2-}$ in the second reaction. The coefficient in front of $\text{I}_2$ is twice the coefficient in front of ${\text{S}_2\text{O}_3}^{2-}$ . How many moles of ${\text{S}_2\text{O}_3}^{2-}$ does each mole of $\text{I}_2$ consume? Two. 0.0060 moles of $\text{I}_2$ will be produced. As a result, $2 \times 0.0060 = 0.0120$ moles of ${\text{S}_2\text{O}_3}^{2-}$ will be needed.

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3 years ago

Need help please! Theres three parts to this that I don't understand at all

butalik [34]

Answer:

Chemical reaction B governs the process

Explanation:

The first part of the question asks to convert the mass of the calcium carbonate given to number of moles.

Mathematically;

Number of moles = mass/molar mass

Molar mass of CaCO3 = 100 g/mol

So the number of moles of CaCO3 will be 2.49/100 = 0.0249 moles

The second part of the question asks to convert the mass of carbon iv oxide to moles of carbon iv oxide

Mathematically;

That is same as ;

Number of moles = mass/molar mass

molar mass of CO2 is 44 g/mol

Number of moles of CO2 = 1.13/44 = 0.0256 moles

Now, if we compare the values of these number of moles, we can see that there are almost equal.

What this means is that the number of moles of calcium carbonate reacted is equal to the number of moles of carbon iv oxide produced.

So what we conclude here is that we have an equal mole ratio between the two compounds.

So the reaction that would be the correct answer will present equal number of moles of carbon iv oxide and calcium carbonate

Thus, we can see that reaction B is the one that governs this process as it is the only reaction out of the three options that present the two compounds with equal number of moles.

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3 years ago

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nikitadnepr [17]

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3 years ago

If this compounds (N2O) molecular mass is 88g are the empirical and molecular formulas the same as one another or different

Softa [21]

Answer:

Explanation:

Let us examine this problem carefully:

Given compound is N₂O

Molecular mass = 88g

Now,

The empirical formula is the simplest formula of a compound.

The molecular formula is the true formula of the compound that shows that actual ratios of the atoms in a compound.

To find if they both have the same molecular and empirical formula, they must have the same molecular mass.

For N₂O;

Molecular mass = 2(14) + 16 = 44g/mole

But the true and given molecular formula of the compound is 88g/mole

This shows that the compound given is the empirical formula of the compound.

Molecular formula:

molecular mass of empirical formula x n = molecular mass of molecular formula

n = $\frac{88}{44}$ = 2

Molecular formula of compound = 2(N₂O) = N₄O₂

Therefore the empirical and molecular formulas are not the same

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