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4 years ago

4P + 502 → 2P20x

Chemistry

1 answer:

Thepotemich [5.8K]4 years ago

6 0

Answer:

Explanation:

According to the Law of Conservation of Matter, the mass of the products in a chemical reaction must equal the mass of the reactants.

5O2 = 10 Oxygen atoms

In 2POx there must be 10 Oxygen atoms too. => x = 5

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Hope it can help you.

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How many atoms are in 2.32 mol2.32 mol of copper?

madreJ [45]

Answer:

since 1 mole = 6.022×10^23

hence in 2.32 moles no. of atoms= 6.022×10^23 × 2.32

13.97104 ×10^23

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3 years ago

4. Will competition for food increase or decrease carrying

melisa1 [442]

Increase

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3 years ago

Gases emitted during volcanic activity often contain high concentrations of hydrogen sulfide and sulfur dioxide. these gases may

kompoz [17]

There can be three possible answers to this question: the amount of moles of SO₂ gas needed to react with 6.41 mol H₂S, and the amount of S and H₂O gas produced.

Amount of SO₂:
6.41 mol H₂S (1 mol SO₂/2 mol 2 mol H₂S) = 3.205 moles SO₂ gas

Amount of S:
6.41 mol H₂S (3 mol S/2 mol 2 mol H₂S) = 9.615 moles S solid

Amount of H₂O:
6.41 mol H₂S (2 mol H₂O/2 mol 2 mol H₂S) = 6.41 moles H₂O gas

7 0

4 years ago

The foul odor of rancid butter is due largely to butyric acid, a compound containing carbon, hydrogen, and oxygen. Combustion an

Firlakuza [10]

Answer: The empirical formula for the given compound is $C_2H_4O$

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=8.59g$

Mass of $H_2O=3.52g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 8.59 g of carbon dioxide, $\frac{12}{44}\times 8.59=2.34g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 3.52 g of water, $\frac{2}{18}\times 3.52=0.391g$ of hydrogen will be contained.

For calculating the mass of oxygen:

Mass of oxygen in the compound = $(4.30g)-[(2.34g)+(0.391g)]=1.57g$

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{2.34g}{12g/mole}=0.195moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.391g}{1g/mole}=0.391moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1.57g}{16g/mole}=0.0981moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is $0.0981$ moles.

For Carbon = $\frac{0.195}{0.0981}=1.98\approx 2$

For Hydrogen = $\frac{0.391}{0.0981}=3.98\approx 4$

For Oxygen = $\frac{0.0981}{0.0981}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : O = 2 : 4 : 1

Hence, the empirical formula for the given compound is $C_2H_4O_1=C_2H_4O$

8 0

3 years ago

An element has three naturally occurring isotopes. ten percent (.10) occurs as 55^x, fifteen percent (.15) occurs as isotope 56^

Leviafan [203]

The average atomic weight is, from the name itself, the average weight of all its naturally occurring isotopes. All you have to do is multiple the abundance of each isotope with its individual mass, then add them altogether.

Mass = (0.10*55)+(0.15*56)+(.75*57)
Mass = 56.65 amu

5 0

4 years ago