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3 years ago

WILL GIVE BRAINLIEST! Calculate the bond for CO2

Chemistry

1 answer:

yawa3891 [41]3 years ago

5 0

Answer:

Bonding Order = number of bonding electrons – number of antibonding electrons/2.

So for CO2, there is a total of 16 electrons, 8 of which are antibonding electrons.

So 16 – 8 = 8; divided by 2 = 4. So, 4 is the bonding order of CO2. The molecular structure of CO2 looks like this:

..~-~~..

O=C=O

..~-~~..

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Which of these is true of sound waves?

9966 [12]

Answer:

Explanation:

3 0

3 years ago

If a steel container holds 3.50 moles of hydrogen gas and 3.50 moles of helium gas, and the total pressure is 4.00 atm., what is

Sunny_sXe [5.5K]

Answer:

1. Partial pressure of H₂ = 2 atm

2. Partial pressure of He = 2 atm

Explanation:

The following data were obtained from the question:

Mole of H₂ = 3.50 moles

Mole of He = 3.50 moles

Total pressure (Pₜ) = 4 atm

Partial pressure of H₂ =?

Partial pressure of He =?

Next, we shall determine the mole fraction of each gas this can be obtained as follow:

Mole of H₂ = 3.50 moles

Mole of He = 3.50 moles

Total mole = Mole of H₂ + Mole of He

Total mole = 3.50 + 3.50

Total mole = 7 moles

Mole fraction of H₂ = mole of H₂ / Total mole

Mole fraction of H₂ = 3.5/7

Mole fraction of H₂ = 0.5

Mole fraction of He = mole of He / Total mole

Mole fraction of He = 3.5/7

Mole fraction of He = 0.5

1. Determination of the partial pressure of H₂.

Mole fraction of H₂ = 0.5

Total pressure (Pₜ) = 4 atm

Partial pressure of H₂ =?

Partial pressure of H₂ = Mole fraction of H₂ × Pₜ

Partial pressure of H₂ = 0.5 × 4

Partial pressure of H₂ = 2 atm

2. Determination of the partial pressure of He.

Total pressure (Pₜ) = 4 atm

Partial pressure of H₂ = 2 atm

Partial pressure of He =?

Total pressure (Pₜ) = Partial pressure of H₂ + Partial pressure of He

4 = 2 + Partial pressure of He

Collect like terms

Partial pressure of He = 4 – 2

Partial pressure of He = 2 atm

6 0

3 years ago

Ammonium nitrate decomposes to dinitrogen monoxide and water. If given 45.7 grams of ammonium

statuscvo [17]

Answer:

20.54 g of H₂O

Explanation:

Since you already have a balanced equation, the next step is to see the ratio between the ammonium nitrate and water in the equation:

NH4NO3(s)—N2O(g)+2H2O

1 mole of ammonium nitrate produces 2 moles of H2O

So we have the ration:

$\dfrac{1\;mole\;of\;NH_4NO_3}{2\;moles\;of\;H_{2}O}$

Let's leave that for later use.

Next step is to covert the mass given into moles. We do that by getting the molar mass of the given and using that as a conversion factor:

Element number of molar mass

atoms of each element

N = 2 x 14.01 g/mole = 28.02 g/mole

H = 4 x 1.01 g/mole = 4.01 g/mole

O = 3 x 16.00 g/mole = <u>48.00 g/mole </u>

80 .03 g/mole

Now we can convert:

$45.7g\;of\;NH_4NO_3\times\dfrac{1\;of\;NH_4NO_3}{80.03\;g\;of\;NH_4NO_3}=0.57\;moles\;of\;NH_4NO_3$

Now we can use this to determine how many moles of H2O this would produce by using the ration we solved for earlier.

$0.57\;moles\;of\;NH_4NO_3\times\dfrac{2\;moles\;of\;H_{2}O}{1\;mole\;of\;NH_4NO_3} =1.14\;moles\;of\;H_{2}O$

And we convert that by getting the molecular mass of H2O, which is 18.02 g/mole:

$1.14\;moles\;of\;H_{2}O\times\dfrac{18.02\;g\;of\;H_{2}O}{1\;\;mole\;of\;H_{2}O} =20.54\;g\;of\;H_{2}O$

But this is only if the whole 45.7 g of ammonium nitrate is used up.

8 0

3 years ago

Which is a discontinued variation: height, eye colour or weight

Natasha2012 [34]

Answer:

Eye colour

Explanation:

6 0

3 years ago

Why is it necessary to maintain excess bromine in the reaction mixture with trans-cinnamic acid and bromine

DerKrebs [107]

Answer:

It is necessary because Trans-cinnamic is a limiting reagent in the mixture reaction while Bromine is the excess reagent

Explanation:

It is necessary to maintain excess bromine in the reaction mixture because Bromine is the excess reagent in the reaction mixture and if it's quantity is less it would consume the limiting reagent ( Trans-cinnamic ) completely . hence Bromine should maintain excess quantity in the reaction mixture

4 0

3 years ago