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NISA [10]
3 years ago
6

Silicate particles from a construction site float through a heavily forested site and then make it into the upper troposphere wh

ere they become larger and gain a high organic carbon content. Explain what happened, with some reactions.
Chemistry
1 answer:
vivado [14]3 years ago
7 0

Answer:

There are two explanations to this: covalent network bonding and carbon-silicate cycle.

Explanation:

A network solid or covalent network solid is a chemical compound which is formed through a continued network of atoms or molecules held together by a covalent bond throughout the system. An example included C-C bond in graphite or C-Si bond in silicon carbide (tentative reaction equation below):

xSiO2 + yCO2→ SixCyO(2x+2y)

Si-Si bonds are not as strong as C-C bonds and can easily be displaced as the particles react with atmospheric CO2.

The second scenerio is when silicates such as calcium silicate CaSiO3, or wollastonite, reacts with atmospheric carbon dioxide and water to yield a calcium ion, Ca2+, a bicarbonate ion, HCO3-, and dissolved silica. This process occurs during carbon-silicate cycle and increase organic carbon content:

2CO2 + H2) + CaSiO3 → + SiO2CaCO3 + CO2 + H2)

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3 years ago
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A 5.00-g sample of copper metal at 25.0 °C is heated by the addition of 133 J of energy. The final temperature of the copper is
vekshin1

<u>Answer:</u> The final temperature of the copper is 95°C.

<u>Explanation:</u>

To calculate the final temperature for the given amount of heat absorbed, we use the equation:

Q= m\times c\times \Delta T

Q = heat absorbed  = +133 J (heat is added to the system)

m = mass of copper = 5.00 g

c = specific heat capacity of copper = 0.38 J/g ° C      

\Delta T={\text{Change in temperature}}=T_2-T_1

T_1=25^oC

Putting values in above equation, we get:

+133J=5.00g\times 0.38J/g^oC\times (T_2-25)\\\\T_2=95^oC

Hence, the final temperature of the copper is 95°C.

3 0
3 years ago
A particular first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0°C. What is the magnitude of k at 95.0°C if Ea =
never [62]

Answer:

k ≈ 9,56x10³ s⁻¹

Explanation:

It is possible to solve this question using Arrhenius formula:

ln\frac{k2}{k1} = \frac{-Ea}{R} (\frac{1}{T2} -\frac{1}{T1} )

Where:

k1: 1,35x10² s⁻¹

T1: 25,0°C + 273,15 = 298,15K

Ea = 55,5 kJ/mol

R = 8,314472x10⁻³ kJ/molK

k2 : ???

T2: 95,0°C+ 273,15K = 368,15K

Solving:

ln\frac{k2}{k1} = 4,257

\frac{k2}{k1} = 70,593

{k2} = 9,53x10^3 s^{-1}

<em>k ≈ 9,56x10³ s⁻¹</em>

I hope it helps!

5 0
3 years ago
According to the following reaction, how many grams of water are produced in the complete reaction of grams of sulfuric acid?
Natasha2012 [34]

This question requires the mass of sulfuric acid and a balance equation. The complete question is given below

Question:

According to the following reaction, how many grams of water are produced in the complete reaction of 24.1 grams of sulfuric acid?

H₂SO₄(aq) + Zn(OH)₂(s) ---------> ZnSO₄(aq) + 2H₂O(l)

Answer:

8.85 grams of water is obtained from 24.1 grams of sulfuric acid according to the given reaction

Explanation:

In this problem, the mass of water can be determined by using the balanced chemical equation.

Step 1: Write all data

Molar mass of water = 18 g

Molar mass of sulfuric acid = 98 g

Given mass of sulfuric acid = 24.1 g

Mass of water from reaction = ?

Step 2: Write statement for conversion

Given equation shows that

1 mole of H₂SO₄ gives 2 moles of water

Step 3: Convert moles into molar mass

Convert the moles into molar mass so, the statement becomes,

98 g of H₂SO₄ gives (2)(18) g of water

1 g of H₂SO₄ gives (2)(18)/98 g of water

Step 4: Use given data

24.1 g of H₂SO₄ gives (2)(18)(24.1)/98 g of water

amount of water = 8.85 g

5 0
3 years ago
Someone help me with chemistry on my account/page please :))
Gemiola [76]

Answer:

ok

Explanation:

5 0
3 years ago
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