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posledela
3 years ago
12

Many pollutants from coal-fired power plants are properly managed today. Which of the following is currently considered to be th

e biggest threat to the environment? Many pollutants from coal-fired power plants are properly managed today. Which of the following is currently considered to be the biggest threat to the environment? carbon dioxide sulfur dioxide nitrous oxide oxygen methane gas
Chemistry
1 answer:
sammy [17]3 years ago
5 0

Answer:

Sulfur dioxide

Explanation:

Sulfur dioxide (SO₂) is a colorless gas, which comes from burning fossil fuels like burning coal, oil and diesel from vehicles. This gas is also released into the environment through volcanic eruptions.

Sulfur dioxide is considered one of the worst air pollutants, mainly because it accumulates in droplets in the air and also because it reacts with other compounds in the atmosphere, forming particulate materials.

This gas is a major contributor to the warming of the planet. Its presence in acid rain (which makes it return from the atmosphere to the earth) is dangerous for plants and animals, in addition to corroding some materials and affecting monuments, buildings, statues.

Acid rain generated by SO₂ and other compounds can lower the pH of lakes and reduce fish populations. In plants, vegetables and flowers, it compromises production and growth.

In humans, sulfur dioxide can cause acute and chronic health effects, especially on the respiratory system, in addition to aggravating cardiovascular problems due to the simultaneous presence of SO₂ and particles in the atmosphere.

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Meera added blue copper sulphate crystals to some water in a beaker.
professor190 [17]

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The solid crystals disappeared

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7 0
4 years ago
The photodissociation of ozone by ultraviolet light in the upper atmosphere is a first-order reaction with a rate constant of 1.
atroni [7]

Answer:

[O₃]= 8.84x10⁻⁷M  

Explanation:

<u>The photodissociation of ozone by UV light is given by:</u>

O₃ + hν → O₂ + O (1)

<u>The first-order reaction of the equation (1) is:</u>

rate = k [O_{3}] = - k \frac{\Delta [O_{3}]}{\Delta t} (2)

<em>where k: is the rate constant and Δ[O₃]/Δt: is the variation in the ozone concentration with time, and the negative sign is by the decrease in the reactant concentration </em>    

<u>We can get the following expression of the </u><u>first-order integrated law</u><u> of the reaction (1), by resolving the equation (2):</u>

[O_{3}]_{t} = [O_{3}]_{0} \cdot e^{-kt} (3)

<em>where [O₃](t): is the ozone concentration in the elapsed time and [O₃]₀: is the initial ozone concentration</em>

We can calculate the initial ozone concentration using equation (3):  

[O_{3}]_{t} = 5.0 \cdot 10^{-3}M \cdot e^{-(1.0\cdot 10^{-5}s^{-1}) (\frac{10d \cdot 24h \cdot 3600 s}{1d \cdot 1h})} = 8.84 \cdot 10^{-7}M

So, the ozone concentration after 10 days is 8.84x10⁻⁷M.

I hope it helps you!                    

3 0
4 years ago
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ICE Princess25 [194]

Answer:

The person who just wanted points is annoying

Explanation:

WHY WOULD YOU DO THAT

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