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2 years ago

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Why wasn't oxidation type chemical weathering common more than 2 billion years ago?

1 answer:

scZoUnD [109]2 years ago

6 0

Answer:

Due to deficiency of Oxygen in atmosphere.

Explanation:

Oxidation is defined in two ways, 1) The addition of Oxygen and Removal of Hydrogen 2) The removal of electrons.

We will discuss the first definition for this question. The addition of oxygen to various compounds results in the oxidation of that compound.

Example: Oxidation of Methane;

CH₄ + 2 O₂ → CO₂ + 2 H₂O

In this example oxygen is added to methane and hydrogen is being removed from methane.

Oxidation type chemical weathering common more than 2 billion years ago because of less amount of Oxygen in atmosphere and the oxygen which was produced by plants reacted with different metals like Iron forming precipitates which precipitated to the bottom of oceans.

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If 60.0 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298 K) and decompose completely via the e

Tresset [83]

Answer:

The final pressure of the carbon dioxide gas will 11.84 atm.

Explanation:

Moles of carbonic acid = $\frac{60.0 g}{62 g/mol}=0.9677 mol$

$H_2CO_3(aq)\rightarrow H_2O(l) + CO_2(g)$

According to reaction, 1 mol of carbonic acid gives 1 mole of carbon dioxide gas.

Then 0.9677 moles of carbonic acid will give :

$\frac{1}{1}\times 0.9677 mol=0.09677 mol$ of carbon dioxide

Moles of carbon dioxide gas = n = 0.09677 mol

Volume of soda bottle = $V_1=2 L$

Pressure of the carbon dioxide gas = P

Temperature of the carbon dioxide gas = T = 298 K

$PV=nRT$ (ideal gas law)

$P=\frac{nRT}{V}=\frac{0.9677 mol\times 0.0821 atm L/mol K\times 298 K}{2 L}=11.84 atm$

The final pressure of the carbon dioxide gas will 11.84 atm.

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2 years ago

Which of the following releases the greatest amount of energy as it proceeds? Assume the same mass of starting material is used

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Chemical reaction is the answer

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Which of the following reactions would you find in a radioisotope thermal generator

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2Al + 3H2SO4 -> Al2(SO4)3 + 3H2How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with alumi

bazaltina [42]

Answer:

290.82g

Explanation:

The equation for the reaction is given below:

2Al + 3H2SO4 -> Al2(SO4)3 + 3H2 now, let us obtain the masses of H2SO4 and Al2(SO4)3 from the balanced equation. This is illustrated below:

Molar Mass of H2SO4 = (2x1) + 32 + (16x4) = 2 + 32 +64 = 98g/mol

Mass of H2SO4 from the balanced equation = 3 x 98 = 294g

Molar Mass of Al2(SO4)3 = (2x27) + 3[32 + (16x4)]

= 54 + 3[32 + 64]

= 54 + 3[96] = 54 + 288 = 342g

Now, we can obtain the mass of aluminium sulphate formed by doing the following:

From the equation above:

294g of H2SO4 produced 342g of Al2(SO4)3.

Therefore, 250g of H2SO4 will produce = (250 x 342)/294 = 290.82g of Al(SO4)3

Therefore, 290.82g of aluminium sulphate (Al(SO4)3) is formed.

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