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3 years ago

What is the mass of 2.15 liters of N2 gas at STP?

Chemistry

2 answers:

Musya8 [376]3 years ago

5 0

Explanation: molar mass of N2=28

Volume occupied at stp=22.4 so 28/22.4=1.25 so mass nitrogen will be 56 multiply 1.25 =70g

IgorLugansk [536]3 years ago

4 0

Answer: 2.68 grams

Explanation:

According to avogadro's law, 1 mole of the substance occupies 22.4 liters at STP and contains avogadro's number $6.023\times 10^{23}$ of particles and weighs equal to its molecular mass.

1 mole of $N_2$ weighs 28 grams.

Also 1 mole of $N_2$ occupies 22.4 Liters.

Thus 22.4 L $N_2$ weigh = 28 grams

2.15 L of $N_2$ weigh = $\frac{28}{22.4}\times 2.15=2.68g$

Thus the mass of nitrogen gas is 2.68 grams.

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How many total electrons are shared between two nitrogen atoms when they bond to form a diatomic nitrogen molecule?

GuDViN [60]

Explanation:

Diatomic Nitrogen molecule means the two atoms of nitrogen $N_{2}$ .

A single nitrogen contains 5 electrons in its valence shell which has 3 single electrons and one pair of electron. When the bond is being made the three single electrons makes the covalent bond with the 3 electrons of other atom which results in 3 pairs . The total electrons shared between the atoms are 3 pairs (6 electrons) . while when it completes the octate the $N_{2}$ is formed.

Nitrogen is colorless, odorless, tasteless and the inert diatomic gas.Nitrogen combines of near about 78% of Earth's atmosphere.It is non-flammable which does not support combustion , it occurs in all living organisms. Nitrogen is used in most of the Biological processes and also used in the formation of fertilizers, in the form of ammonia and ammonia based compounds.It is also used in Chemical Industries for making nylon , explosives, dyes and etc. The breathing of Nitrogen is deadly, as it displaces the oxygen.

8 0

3 years ago

Help please

kipiarov [429]

The correct options are these:

1. It will follow the law of conservation of mass.

2.The mass of products will be equal to the mass of the reactants.

The law of conservation of mass states that ' matter can neither be created nor destroyed. Thus, if a chemical equation is balanced, the mass of the reactant at the beginning of the reaction will be equal to the mass of the product after the reaction. This shows that the chemical reaction obeys the law of conservation of mass.

6 0

3 years ago

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Iron(111)Carbonate +cesium > cesium carbonate +iron balced

ipn [44]

Balanced chemical equation for the given reaction is Fe₂(CO₃)₃ + 6Cs → 3Cs₂CO₃ + 2Fe.

<h3>What is balanced equation?</h3>

Balanced chemical equations are those equations in which all entities are present in equal amount on reactant side as well as on product side.

Given balanced chemical reaction is:
Fe₂(CO₃)₃ + 6Cs → 3Cs₂CO₃ + 2Fe

Above given equation is a balanced chemical equation where all atoms of reactant as well as of products are present in same amount.

Hence, required balanced equation is Fe₂(CO₃)₃ + 6Cs → 3Cs₂CO₃ + 2Fe.

To know more about balanced chemical reaction, visit the below link:
brainly.com/question/26694427

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2 years ago

How many moles are in 25 grams of HF

sergey [27]

Using this equation, we can take 25/(1.0 + 19) and find that it is equal to 1.25 moles.

5 0

3 years ago

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In a particular experiment, 2.50-g samples of each reagent are reacted. The theoretical yield of lithium nitride is ________ g.

Neporo4naja [7]

Answer:

4.18 g

Explanation:

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Given: For Li

Given mass = 2.50 g

Molar mass of Li = 6.94 g/mol

<u>Moles of Li = 2.50 g / 6.94 g/mol = 0.3602 moles</u>

Given: For $N_2$

Given mass = 2.50 g

Molar mass of $N_2$ = 28.02 g/mol

<u>Moles of $N_2$ = 2.50 g / 28.02 g/mol = 0.08924 moles</u>

According to the given reaction:

$6Li+N_2\rightarrow 2Li_3N$

6 moles of Li react with 1 mole of $N_2$

1 mole of Li react with 1/6 mole of $N_2$

0.3602 mole of Li react with $\frac {1}{6}\times 0.3602$ mole of $N_2$

Moles of $N_2$ that will react = 0.06 moles

Available moles of $N_2$ = 0.08924 moles

$N_2$ is in large excess. (0.08924 > 0.06)

Limiting reagent is the one which is present in small amount. Thus,

Li is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

6 moles of Li gives 2 mole of $Li_3N$

1 mole of Li gives 2/6 mole of $Li_3N$

0.3602 mole of Li react with $\frac {2}{6}\times 0.3602$ mole of $Li_3N$

Moles of $Li_3N$ = 0.12

Molar mass of $Li_3N$ = 34.83 g/mol

Mass of $Li_3N$ = Moles × Molar mass = 0.12 × 34.83 g = 4.18 g

<u>Theoretical yield = 4.18 g</u>

5 0

3 years ago