full valence shells
when they have satisfied the octet rule naturally or through bonding to obtain full valence shells
when their valence electrons have "fallen" back to ground state through bonding
Answer:
when they have satisfied the octet rule naturally or through bonding to obtain full valence shells
Explanation:
Generally, most atoms of an element are unstable because they have a void in their electron shell to fill, hence, they need to react with other elements to fulfil this task of octet.
Octet rule states that atoms of elements engage in reactions to form compounds so they can have eight (8) valence electrons in their shell. Noble gases e.g argon, neon etc. are elements that have naturally satisfied this octet rule by possession of 8 valence electrons in their shell. Other elements that do not have this naturally becomes reactive and enter bonding with other atoms to obtain full valence shells.
Answer:
The partial pressure of nitrogen is 0.402 atm.
Explanation:
Given data:
Number of moles of helium = 1 mol
Number of moles of nitrogen = 2 mol
Total pressure of mixture = 0.60 atm
Partial pressure of nitrogen = ?
Solution:
First of all we will calculate the mole fraction of nitrogen.
mole fraction of nitrogen = moles of nitrogen / total number of moles
mole fraction of nitrogen = 2 mol / 3 mol = 0.67
Partial pressure of nitrogen:
P₁ = [ n₁ /n(t)] × Pt
P₁ = 0.67 × 0.60 atm
P₁ = 0.402 atm
To find the partial pressure of nitrogen in a mixture, calculate the mole fraction of nitrogen and multiply it by the total pressure of the mixture. In this case, the partial pressure of nitrogen is 0.40 atm.
The question is about determining the partial pressure of nitrogen in a mixture of helium and nitrogen based on Dalton's Law of Partial Pressures. First, we find the mole fraction of nitrogen, which is the ratio of moles of nitrogen to the total moles in the mixture. In this scenario, the mole fraction (XN2) is 2 moles of nitrogen divided by the total moles (1 mole of helium + 2 moles of nitrogen), which equals 2/3.
Then we use Dalton's Law, which states that the partial pressure of nitrogen (PN2) can be found by multiplying the mole fraction by the total pressure of the mixture. Therefore, the partial pressure of nitrogen is 0.60 atm (total pressure) multiplied by 2/3 (mole fraction of nitrogen), yielding a partial pressure for nitrogen of 0.40 atm.
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b) increasing the temperature helps dissolve more flavoring
c) increasing the surface area helps dissolve more flavoring
d) decreasing agitation helps dissolve more flavoring
In order for you to calculate for the mass of ammonium carbonate, you need to know the molar mass of it and the nitrogen atoms in the compound. Ammonium carbonate has a molar mass of 96.08 grams per mole. There are two nitrogen atoms in ammonium carbonate which is equal to 28.02 grams per mole. Divide the molar mass of nitrogen to the ammonium carbonate, 28.02/96.08 x 100, we get 29.16wt% nitrogen.
Answer:
29.16%.
Explanation:
You can determine the mass percent, or how much of the total mass of ammonium carbonate is nitrogen, by first determining the mass of nitrogen and the mass of the total compound.
1. the mass of nitrogen in this compound is 2 x 14.007, or 28.014.
2. the mass of ammonium carbonate is 96.09 grams.
To find the percentage of nitrogen in the overall mass of ammonium carbonate, simply divide the mass of nitrogen by the mass of ammonium carbonate and multiply by 100:
28.014/96.09 x 100 ....................... 29.16%.
Also, I got the correct answer :)