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eduard
2 years ago
11

When reacted with elemental chlorine at room temperature, liquid phosphorous trichloride (PCl3) is converted to solid phosphorou

s pentachloride (PCl5).
Chemistry
1 answer:
Sergeu [11.5K]2 years ago
6 0

PCl₅ reacts upon contact with water to launch hydrogen chloride and supply phosphorus oxides. the primary hydrolysis product is phosphorus oxychloride     PCl₅ + H₂O ========>  POCl₃ + 2HCl.

Phosphorus trichloride appears as a colorless or slightly yellow fuming liquid with a pungent and irritating odor resembling that of hydrochloric acid. Causes severe burns to skin, eyes and mucous membranes.

Divide the mass of the material through its molar mass. The molar mass of a substance is the mass in grams of 1 mole of that substance. This mass is given via the atomic weight of the chemical unit that makes up that substance in atomic mass units.

One mole is described as the amount of substance containing as many number one entities atoms, molecules, ions, electrons, radicals, and lots of others. As there are atoms in 12 grams of carbon - 12(6. 023×10²³. The mass of one mole of a substance equals to its relative molecular mass expressed in grams.

Learn more about  phosphorous trichloride here:-brainly.com/question/2626850

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What is the answer pls help me
scZoUnD [109]
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3 0
3 years ago
When 11.12 g of neon is combined in a 100 L container at 80oC with 9.59 g of argon, what is the mole fraction of argon?
PolarNik [594]
The correct answer for the question that is being presented above is this one: "<span>0.3."

Here it is how to solve.
M</span><span>olecular mass of Ar = 40
</span><span>Molecular mass of Ne = 20
</span><span>Number of moles of Ar = 9.59/40 = 0.239
</span><span>Number of moles of Ne = 11.12/20= 0.556
</span><span>Mole fraction of argon = 0.239/ ( 0.239 + 0.556) = 0.3</span><span>
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3 0
4 years ago
I WILL GIVE BRAINLIEST!!!!!!!!
docker41 [41]
You can calculate the excess reactant by subtracting the mass of excess reagent consumed from the total mass of reagent given therefore,
The answer: Theoretical yield is 121.60 g of NH₃
Excess reactant is H₂
Rate limiting reactant is N₂
explanation: 100 g of Nitrogen
100 g of hydrogen
We are required to identify the theoretical yield of the reaction, the excess reactant and the rate limiting reagent.
We first write the equation for the reaction between nitrogen and hydrogen;
N₂ + 3H₂ → 2NH₃
From the reaction 1 mole of nitrogen reacts with 3 moles of Hydrogen gas.
Secondly we determine the moles of nitrogen gas given and hydrogen gas given;
Moles of Nitrogen gas
Moles = Mass ÷ Molar mass
Molar mass of nitrogen gas = 28.0 g/mol
Moles of Nitrogen gas = 100 g ÷ 28 g/mol 3.57 moles
Moles of Hydrogen gas
Molar mass of Hydrogen gas = 2.02 g/mol
Moles = 100 g ÷ 2.02 g/mol
= 49.50 moles
From the mole ratio given by the equation, 1 mole of nitrogen requires 3 moles of Hydrogen gas.
Thus, 3.57 moles of Nitrogen gas requires (3.57 × 3) 10.71 moles of Hydrogen gas.
This means, Nitrogen gas is the rate limiting reagent and hydrogen gas is the excess reactant.
Third calculate the theoretical yield of the reaction.
1 mole of nitrogen reacts to from 2 moles of ammonia gas
Therefore;
Moles of ammonia gas produced = Moles of nitrogen × 2
= 3.57 moles × 2
= 7.14 moles
But; molar mass of Ammonia gas is = 17.03 g/mol
Therefore;
Mass of ammonia gas produced = 7.14 moles × 17.03 g/mol
= 121.59 g
= 121.60 g
Thus, the theoretical amount of ammonia gas produced is 121.60 g
3 0
2 years ago
. A large quantity of very dilute aqueous HCl solution is neutralized by the addition of the stoichiometric amount of a 10-mol-%
ad-work [718]

Answer:

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Explanation:

5 0
3 years ago
What is 1006 in scientific notation?
vladimir1956 [14]

Answer:

1.006 * 103

Explanation:

Add the number between 1 and 9 and add a decimal accordingly . so the answer is 1.006 multiplied by 10 raised to power 3

8 0
3 years ago
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