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4 years ago

Identify the bond with the highest bond energy. identify the bond with the highest bond energy. c=c si=o c=n n=n o=o

1 answer:

8 0

Ans- bond with the highest bond energy is for ( C=C \rightarrow 620 (kJ/mol) N=N \rightarrow 418 (kJ/mol) Si=O \rightarrow 452 (kJ/mol) O=O \rightarrow 498.7 (kJ/mol) C=N \rightarrow 615 (kJ/mol) C=C \rightarrow 620 (kJ/mol)

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Natasha_Volkova [10]

Answer:

At the nucleus point of a substance, the particles have enough kinetic energy to break free from their fixed positions.

Answer : nucleus

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2 years ago

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AlekseyPX

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3 years ago

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In the background information, it was stated that CaF2 has solubility, at room temperature, of 0.00160 g per 100 g of water. How

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Answer:

2.05*10⁻⁵ moles of CF₂ can dissolve in 100 g of water.

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Explanation:

First, by definition of solubility, in 100 g of water there are 0.0016 g of CaF₂. So, to know how many moles are 0.0016 g, you must know the molar mass of the compound. For that you know:

Ca: 40 g/mole
F: 19 g/mole

So the molar mass of CaF₂ is:

CaF₂= 40 g/mole + 2*19 g/mole= 78 g/mole

Now you can apply the following rule of three: if there are 78 grams of CaF₂ in 1 mole, in 0.0016 grams of the compound how many moles are there?

$moles=\frac{0.0016 grams*1 mole}{78 grams}$

moles=2.05*10⁻⁵

2.05*10⁻⁵ moles of CF₂ can dissolve in 100 g of water.

Now, to answer the following question, you can apply the following rule of three: if by definition of density in 1 mL there is 1 g of CaF₂, in 1000 mL (where 1L = 1000mL) how much mass of the compound is there?

$mass of CaF_{2}=\frac{1000 mL*1g}{1mL}$

mass of CaF₂= 1000 g

Now you can apply the following rule of three: if there are 78 grams of CaF₂ in 1 mole, in 1000 grams of the compound how many moles are there?

$moles=\frac{1000 grams*1 mole}{78 grams}$

moles=12.82

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3 years ago

Another name for light is

Karo-lina-s [1.5K]

Answer:

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I hope this helps!

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2 years ago

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Gemiola [76]

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4 years ago

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