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Aleks [24]
3 years ago
7

What is coal combustion

Chemistry
1 answer:
Musya8 [376]3 years ago
4 0

Answer:

  • <em>Coal combustion</em> is burning coal to produce electricity, but it releases a lot of pollutants to the atmosphere.

Explanation:

<em>Coal combustion</em> is the process of burning coal to produce energy: the combustion releases heat which is used to heat water, producing steam which is used to move turbines and produce electricity.

The chemical equation for the combustion of pure coal is:

     C(s)+O_2(g)\rightarrow CO_2+heat

That is called complete combustion.

Incomplete combustion also happens:

      2C(s)+O_2(g)\rightarrow 2CO(g)+heat

CO₂ is a greenhouse gas, thus it is a pollutants.

Also, mined coal contain a lot of other elements, like sulfur (S), nitrogen (N), organic compounds, and heavy metals, which implies many side reactions. So, the combustion of coal releases a lot of pollutants to the atmosphere, which is why this is considered a dirty process.

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what is the boiling point of water at the top of mount everest where the atmospheric pressure is only 34% as strong
Tema [17]

This question is incomplete, the complete is;

Water has a heat of vaporization (ΔHvap) of 44.01 kJ mol-1 and boils at 100 degrees C at sea level.

What is the boiling point of water  at the top of Mount Everest where the atmospheric pressure is only 34% as strong as the pressure at sea level?

Answer: the boiling point of water at the top of mount Everest where the atmospheric pressure is only 34% as strong is 74 °C

Explanation:

Given that;

P1 = 1 atm,

T1 = 100°C =  373 K

P2 = P1 × 34% = 1×0.34 = 0.34 atm

T1 = ?

ΔH = 44.01 kJ mol⁻¹ = 44.01×10³ J/mol

R = 8.314 J/k.mol

now using the Clausius - Clapeyron equation;

p1_∫^p2 d.InP = ΔHvap/R T1_∫^T2. 1/T².dT

⇒ In(P2/P1) = ΔHvap/R (1/T1 - 1/T2)

so we substitute;

ln( 0.34/1 ) = ( 44.01×10³ / 8.314) × ( 1/373 - 1/T2)  

-1.0788 = 5293.4808 × ( 0.00268 - 1/T2)

-1.0788 = 14.1865 - 5293.4808(1/T2)

5293.4808(1/T2) = 14.1865 + 1.0788

5293.4808(1/T2) = 15.2653

(1/T2) = 15.2653 / 5293.4808

(1/T2) = 0.0028837

T2 = 1 / 0.0028837

T2 = 346.8 K

WE convert to Celsius

t2 =346.8 K − 273.15 = 73.65 °C ≈ 74 °C

Therefore, the boiling point of water at the top of mount Everest where the atmospheric pressure is only 34% as strong is 74 °C

8 0
3 years ago
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