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lilavasa [31]
3 years ago
10

Burning wood to power engines and machines ushered in the Industrial Revolution in 1769.Coal became the major fuel in the early

twentieth century and was replaced by petroleum inthe 1950s. Coal (C), natural gas (CH4), and petroleum (mainly octane, C8H18) are themodern-day fossil fuels. Write balanced equations for their reactions with oxygen(combustion) including the amount of heat produced. What is the environmentalsignificance of these changes in sources of energy
Chemistry
1 answer:
Sloan [31]3 years ago
4 0

Answer:

Natural gas combustion equation:

CH4 + O2 ==> CO2 + 2 H2O + HEAT

Octane or oil combustion equation:

2C8H18 + 25 O2 ===> 16CO2 + 18 H2O.

If these fuels were replaced by self-sustaining energy sources, the contamination of the environment would be less, since their combustion generates toxic compounds that damage the ozone layer, promoting the greenhouse effect, increasing the Earth's temperature and also promoting the increase in the passage of ultraviolet radiation.

Explanation:

The combustion reactions are exothermic, and irreversible, they can be complete and incomplete combustions.

They always consist of oxygen as a reagent and water and carbon dioxide as a product (complete), in the case of the incomplete the difference is that the products vary and there may be waste or chemical compounds that failed to burn.

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Explanation:

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In Rutherford's model of the atom, where are the electrons and protons located?
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Why is concentrated sodium hydroxide preferred than water
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8 0
2 years ago
A compound is found to contain 64.80 % carbon, 13.62 % hydrogen, and 21.58 % oxygen by weight. What is the empirical formula for
insens350 [35]

Answer:

Empirical formula is C₄H₁₀O

Explanation:

Values for C, H and O are determined as centesimal composition.

64.80 g of C in 100g of compound

13.62g of H in 100 g of compound

21.58 g of O in 100 g of compound.

We convert the mass to moles:

64.80 g . 1mol/ 12g = 5.4 moles of C

13.62 g . 1 mol /1g = 13.62 moles of H

21.58 g . 1 mol/16g = 1.35 moles of O

We pick the lowest value and we divide:

5.4 moles of C / 1.35 = 4 C

13.62 moles of H / 1.35 = 10 H

1.35 moles of O / 1.35 = 1 O

Empirical formula is C₄H₁₀O, it can be the diethyl ether.

We confirm, the excersise is well done.

Molar mass = 74g/mol

74 g of compound we have (12 . 4)g of C

In 100 g of compound we may have (100 . 48) / 74 = 64.8 g

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