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3 years ago

Preparation of ammonia gas

Chemistry

1 answer:

Makovka662 [10]3 years ago

7 0

Answer:

Ammonia is easily made in the laboratory by heating an ammonium salt, such as ammonium chloride NH4Cl with a strong alkali, such as sodium hydroxide or calcium hydroxide.

The gas may also be made by warming concentrated ammonium hydroxide.

Explanation:

2NH4Cl + Ca(OH)2 → CaCl2 + 2H2O + 2NH3(g)

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Please compare between physical and chemical properties of matter<br>

stealth61 [152]

Answer:

A physical property is a characteristic of a substance that can be observed or measured without changing the identity of the substance. Physical properties include color, density, hardness, and melting and boiling points. A chemical property describes the ability of a substance to undergo a specific chemical change

Explanation:

I got this from chem.libretexts.org in case you wanted to know

5 0

3 years ago

Reaction between silver nitrate and sodium chloride. A balanced chemical equation

Anvisha [2.4K]

Answer:

NaCl(aq) + AgNO3(aq) Sodium Silver chloride nitrate AgCl(s) + NaNO3(aq) Silver Sodium chloride nitrate

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3 years ago

A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as b

AnnyKZ [126]

Answer : The mass percentage of barium in the compound is, 53.8 %

Explanation : Given,

Mass of barium compound = 441 mg

Mass of barium sulfate = 403 mg = 0.403 g (1 mg = 0.001 g)

The balanced chemical reaction will be:

$Ba^{2+}(aq)+Na_2SO_4(aq)\rightarrow BaSO_4(s)+2Na^+(aq)$

First we have to calculate the moles of $BaSO_4$

$\text{Moles of }BaSO_4=\frac{\text{Mass of }BaSO_4}{\text{Molar mass of }BaSO_4}$

Molar mass of $BaSO_4$ = 233.38 g/mole

$\text{Moles of }BaSO_4=\frac{0.403g}{233.38g/mole}=0.001727mole$

Now we have to calculate the moles of barium ion.

From the balanced chemical reaction, we conclude that

As, 1 mole of barium sulfate produced from 1 mole of barium ion

So, 0.001727 mole of barium sulfate produced from 0.001727 mole of barium ion

Now we have to calculate the mass of barium ion.

$\text{ Mass of }Ba^{2+}=\text{ Moles of }Ba^{2+}\times \text{ Molar mass of }Ba^{2+}$

Molar mass of barium = 137.3 g/mol

$\text{ Mass of }Ba^{2+}=(0.001727moles)\times (137.3g/mole)=0.2371g$

Now we convert the mass of barium ion from gram to mg.

Conversion used : (1 g = 1000 mg)

Mass of barium ion = 0.2371 g = 237.1 mg

Now we have to calculate the mass percentage of barium in the compound.

Mass percent of barium = $\frac{237.1mg}{441mg}\times 100=53.8\%$

Thus, the mass percentage of barium in the compound is, 53.8 %

8 0

4 years ago

Question 1

Dominik [7]

The following types of bonds exists between the listed atoms;

Si and O - polar covalent
O and O - Covalent
C and H - Covalent
Li and F - ionic
Ba and S - ionic

<h3>What is a polar covalent bonds?</h3>

A bond is polar covalent when the electronegativity difference between the bonding atoms is above that found in a nonpolar covalent bond. Now we shall see the types of bonds between these atoms.

Si and O - polar covalent
O and O - Covalent
C and H - Covalent
Li and F - ionic
Ba and S - ionic

Learn more about polar covalent bonds:brainly.com/question/10777799

#SPJ1

3 0

2 years ago

Compound a has a pka of 7 and compound b has a pka of 10. compound a is how many times more acidic than compound b?

Pavel [41]

Ka is the acid dissociation equilibrium constant. The larger the value of the Ka, the stronger is the acid. To find Ka from pKa, the equation is:

pKa = -log[Ka]

@pKa = 7
7 = -log[Ka]
Ka = 1×10⁻⁷

@pKa = 10
10 = -log[Ka]
Ka = 1×10⁻¹⁰

This, pKa 7 is more acidic than pKa 10. The scale factor would be:
1×10⁻⁷/1×10⁻¹⁰ = 1,000

<em>Therefore, Compound A is 1,000 times more acidic than Compound B.</em>

4 0

4 years ago

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Preparation of ammonia gas​

Preparation of ammonia gas