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3 years ago

Combustion of fossil fuels contaminated with sulfur leads to what phenomena?

1 answer:

5 0

It leads to acid rain.
The sulfur burns to give sulfur dioxide, then binds with oxygen to give sulfur trioxide. This is turn reacts with water in air to give sulfuric acid. Then it falls as rain, known as acid rain.

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The mass number is equal to which of the following? Question 5 options: Protons + Neutrons Protons + Atomic Number Neutrons + El

Sedbober [7]

Answer: The mass number is the sum of the numbers of protons and neutrons present in the nucleus of an atom.

I hope that this helps you !

7 0

3 years ago

What are the limitations of Bronsted-Lowery concept???

HACTEHA [7]

Answer:

There is no limitation at all because that is the basic theory of solution electrolysis

3 0

3 years ago

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Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel ro

melamori03 [73]

Answer: The mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For nickel:

Given mass of nickel = 14.8 g

Molar mass of nickel = 58.7 g/mol

Putting values in equation 1, we get:

$\text{Moles of nickel}=\frac{14.8g}{58.7g/mol}=0.252mol$

For the given chemical reaction:

$3NiO(s)+2Al(s)\rightarrow 3Ni(l)+Al_2O_3(s)$

For nickel (II) oxide:

By Stoichiometry of the reaction:

3 moles of nickel are produced from 3 moles of nickel (II) oxide

So, 0.252 moles of nickel will be produced from $\frac{3}{3}\times 0.252=0.252mol$ of nickel (II) oxide

Now, calculating the mass of nickel (II) oxide by using equation 1:

Molar mass of nickel (II) oxide = 74.7 g/mol

Moles of nickel (II) oxide = 0.252 moles

Putting values in equation 1, we get:

$0.252mol=\frac{\text{Mass of nickel (II) oxide}}{74.7g/mol}\\\\\text{Mass of nickel (II) oxide}=(0.252mol\times 74.7g/mol)=18.8g$

For aluminium:

By Stoichiometry of the reaction:

3 moles of nickel are produced from 2 moles of aluminium

So, 0.252 moles of nickel will be produced from $\frac{2}{3}\times 0.252=0.168mol$ of aluminium

Now, calculating the mass of aluminium by using equation 1:

Molar mass of aluminium = 27 g/mol

Moles of aluminium = 0.168 moles

Putting values in equation 1, we get:

$0.168mol=\frac{\text{Mass of aluminium}}{27g/mol}\\\\\text{Mass of aluminium}=(0.168mol\times 27g/mol)=4.54g$

Hence, the mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.

4 0

3 years ago

What is the formula for the polyatomic ion and name the following compound Sn(NO2)2

garri49 [273]

There are 9 polyatomic ions so which one and the compound “Sn(NO2)2 is Tin(ll) Nitrite

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3 years ago

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What is the definition of percent composition in your own words?

harkovskaia [24]

Answer:

percentage by mass of each element in a compound.

Explanation:

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2 years ago