Is the reaction balanced?

Explain how the burning of fossil fuels can cause a disruption to the carbon cycle.

TiliK225 [7]

By adding a lot of carbon dioxide of what is necessary could be harmful for living things, the carbon cycle is something natural, this cycle released enough carbon dioxide, as result not to damage living things so by adding more could prejudicial

8 0

3 years ago

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a sample of natural gas contains 8.24 moles of methane, 0.421 moles of ethane, and 0.116 moles of propane. if the total pressure

Varvara68 [4.7K]

The partial pressure (Px) of a gas in a gas mixture is equal to its mole fraction (Xi) multiplied by the total pressure (P) of the gas mixture. That means that we have to calculate the mole fraction of each gas, then calculate its partial pressure. The mole fraction of a gas is its number of moles (n) divided by the total number of moles.

$$ Mole fraction of methane: \\$\chi_{\text {methane }}=\frac{\mathrm{n}_{\text {methane }}}{\mathrm{n}_{\text {total }}} \chi_{\text {methane }}=\frac{8.24 \mathrm{~mol}}{8.24 \mathrm{~mol}+0.421 \mathrm{~mol}+0.116 \mathrm{~mol}} \chi_{\text {methane }}=\frac{8.24 \mathrm{~mol}}{8.78 \mathrm{~mol}} \chi_{\text {methane }}=0.938$

$$Partial Pressure of methane:\\$\mathrm{P}_{\text {methane }}=\chi_{\text {methane }} \times \mathrm{PP}_{\text {methane }}=0.938 \times 1.37 \mathrm{~atm} \mathbf{P}_{\text {methane }}=\mathbf{1 . 2 8} \mathbf{~ a t m}$

$$Mole fraction of ethane: \\$\chi_{\text {ethane }}=\frac{\mathrm{n}_{\text {ethane }}}{\mathrm{n}_{\text {total }}} \chi_{\text {ethane }}=\frac{0.421 \mathrm{~mol}}{8.78 \mathrm{~mol}} \chi_{\text {ethane }}=0.0479$

$$Partial pressure of ethane:\\$\mathrm{P}_{\text {ethane }}=\chi_{\text {ethane }} \times \mathrm{PP}_{\text {ethane }}=0.0479 \times 1.37 \mathrm{~atm} \mathrm{P}_{\text {ethane }}=\mathbf{0 . 0 6 5 6} \mathbf{~ a t m}$

$$Mole fraction of propane:\\$\chi_{\text {propane }}=\frac{\mathrm{n}_{\text {propane }}}{\mathrm{n}_{\text {total }}} \chi_{\text {propane }}=\frac{0.116 \mathrm{~mol}}{8.78 \mathrm{~mol}} \chi_{\text {propane }}=0.0132$

<h3>What is Dalton’s Law?</h3>

Dalton's law of partial pressures is a gas law that states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures exerted by each individual gas in the mixture. The mole fraction of a given gas in a gas mixture is equal to the ratio of the partial pressure of that gas to the total pressure exerted by the gas mixture. This mole fraction can also be used to calculate the total number of moles of constituent gas if the total number of moles of the mixture is known. In addition, the mole fraction can also be used to calculate the volume of a certain gas in a mixtur.

To learn more about Dalton’s Law, visit:

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6 0

11 months ago

Do Halogens gain or lose electrons to form ions

Llana [10]

Halogens are among the most reactive of all elements. They have seven valence electrons, so they are very “eager” to gain one electron to have a full outer energy level. So they gain

4 0

3 years ago

Which is a product in the following chemical reaction? CH4 + 2O2 → CO2 + 2H2O

NeX [460]

<span>CH4 + 2O2 → CO2 + 2H2O
</span>
The products are water (H2O) and carbon dioxide (CO2)

5 0

3 years ago

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The number of hydrogen atoms in 0.050 mol of c3h8o3 is

Natalka [10]

Answer:

2.40 × 10²³ Atoms of Hydrogen

Solution:

The number of hydrogen atoms in C₃H₈O₃ are calculated as;

As, there are eight hydrogen atoms per molecule of C₃H₈O₃, therefore the number of hydrogen atoms per mole of C₃H₈O₃ are calculated as;

1 mole C₃H₈O₃ contains = 6.022 × 10²³ Molecules of C₃H₈O₃

So,

0.05 mole C₃H₈O₃ will contain = X Molecules of C₃H₈O₃

Solving for X,

X = (0.05 × 6.022 × 10²³) ÷ 1

X = 3.011 × 10²² Molecules of C₃H₈O₃

As,

1 Molecule of C₃H₈O₃ contains = 8 Atoms of Hydrogen

So,

3.011 × 10²² Molecules of C₃H₈O₃ will contain = X Atoms of Hydrogen

Solving for X,

X = (3.011 × 10²² × 8) ÷ 1

X = 2.40 × 10²³ Atoms of Hydrogen

6 0

2 years ago