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musickatia [10]
3 years ago
5

PLSSS HELP MEE 100 POINTS!!!!!!! How many atoms of each element does magnesium hydroxide, Mg(OH)2, contain? Magnesium = 1 atom,

Oxygen = 2 atoms, Hydrogen = 2 atoms Magnesium = 2 atom, Oxygen = 2 atoms, Hydrogen = 2 atoms Magnesium = 1 atom, Oxygen = 1 atoms, Hydrogen = 2 atoms Magnesium = 2 atom, Oxygen = 1 atoms, Hydrogen = 2 atoms
Chemistry
2 answers:
Basile [38]3 years ago
5 0

It would be Magnesium = 1 atom, Oxygen = 2 atoms, Hydrogen = 2 atoms. It has 5 atoms total. There is 1 magnesium and you multiply each element by the the 2 outside the parenthesis to get 2 oxygen and 2 hydrogen.

kompoz [17]3 years ago
3 0

how many atoms Mg(OH)2 contains? choices are:

Magnesium = 1 atom, Oxygen = 2 atoms, Hydrogen = 2 atoms

Magnesium = 2 atom, Oxygen = 2 atoms, Hydrogen = 2 atoms

Magnesium = 1 atom, Oxygen = 1 atoms, Hydrogen = 2 atoms

Magnesium = 2 atom, Oxygen = 1 atoms, Hydrogen = 2 atoms


look at Mg(OH)2, there should be 1x Mg, 2x O n 2x H

so ans is A.  Magnesium = 1 atom, Oxygen = 2 atoms, Hydrogen = 2 atoms


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Answer:

The correct option is: stable environment

Explanation:

According to the Darwin's theory, natural selection is the concept by which all the small useful variations of traits are preserved.

According to Darwin, there are three <u>necessary and sufficient conditions</u> for the occurrence of natural selection:

1. struggle for existence

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CH4 with pressure 1 atm and volume 10 liter at 27°C is passed into a reactor with 20% excess oxygen, how many moles of oxygen is
BaLLatris [955]

Answer : The moles of O_2 left in the products are 0.16 moles.

Explanation :

First we have to calculate the moles of CH_4.

Using ideal gas equation:

PV=nRT

where,

P = pressure of gas = 1 atm

V = volume of gas = 10 L

T = temperature of gas = 27^oC=273+27=300K

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R = gas constant = 0.0821 L.atm/mol.K

Now put all the given values in the ideal gas equation, we get:

(1atm)\times (10L)=n\times (0.0821L.atm/mol.K)\times (300K)

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Now we have to calculate the moles of O_2.

The balanced chemical reaction will be:

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From the balanced reaction we conclude that,

As, 1 mole of CH_4 react with 2 moles of O_2

So, 0.406 mole of CH_4 react with 2\times 0.406=0.812 moles of O_2

Now we have to calculate the excess moles of O_2.

O_2 is 20 % excess. That means,

Excess moles of O_2 = \frac{(100 + 20)}{100} × Required moles of O_2

Excess moles of O_2 = 1.2 × Required moles of O_2

Excess moles of O_2 = 1.2 × 0.812 = 0.97 mole

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Moles of O_2 left in the products = Excess moles of O_2 - Required moles of O_2

Moles of O_2 left in the products = 0.97 - 0.812 = 0.16 mole

Therefore, the moles of O_2 left in the products are 0.16 moles.

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