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4 years ago

The boiling point of water is also the same as its' ___________ point

Chemistry

2 answers:

Helga [31]4 years ago

7 0

212°F (100°C) I think

Brrunno [24]4 years ago

7 0

Answer: Steam point

Explanation: Boiling point of water is the temperature at which the

Vapour pressure is the equal to the atmospheric pressure. Boiling point of water depends on atmospheric pressure or surrounding pressure water boils at 100°C but it changes with increase in surrounding temperature. Steam point is also known as the Boiling point.

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Which of the following types of equations will include spectator ions

krek1111 [17]

Answer:- B) Full ionic equation

Explanations:- A molecular equation does not have ions. It is the non charge form of the elements of compounds. When we write the full or total ionic equation for the molecular equation then ions are written for the aqueous species. The ions present on both sides(reactant and product sides) in a full ionic equation are known as spectator ions or common ions. These ions are canceled to get the net ionic equation. For example, reaction of aqueous solution of silver nitrate with aqueous solution of barium chloride to form aqueous solution of barium nitrate and a precipitate of silver chloride.

Balanced molecular equation:-

$BaCl_2(aq)+2AgNO_3(aq)\rightarrow Ba(NO_3)_2(aq)+2AgCl(s)$

Full ionic equation:-

$Ba^+^2(aq)+2Cl^-(aq)+2Ag^+(aq)+2NO_3^-(aq)\rightarrow Ba^+^2(aq)+2NO_3^-(aq)+2AgCl(s)$

If we look at the above full ionic equation then barium ion and nitrate ions are the spectator ions are they are present on both sides.

So, while writing the net ionic equation, these spectator ions are canceled.

Net ionic equation:-

$2Cl^-(aq)+2Ag^+(aq)\rightarrow2AgCl(s)$

So, it is also clear from the above example that it's the full ionic equation that include spectator ions.

6 0

3 years ago

Read 2 more answers

Fe2O3 + Al ---> Fe + Al2O3

PIT_PIT [208]

Answer:

$Fe2O3 + 2Al \rightarrow 2Fe + Al2O3$

Explanation:

Hello!

In this case, when balancing chemical reactions, we must make sure that the atoms of each element are the same at both reactants and products; thus, for the given reaction, we need two iron and aluminum atoms at each side based on their subscripts in the given oxides as shown below:

$Fe2O3 + 2Al \rightarrow 2Fe + Al2O3$

Best regards!

5 0

3 years ago

The air we breathe contains different individual gases (mostly nitrogen and oxygen). Which of the following correctly describes

shusha [124]

Answer:

A. Mixture

Explanation:

Our air has a group of gases. For example, you said nitrogen & oxygen, Which is significantly a mixture.

5 0

3 years ago

At what point does the radiation start to affect satellites in the atmosphere

Aleksandr-060686 [28]

After that have been up for a while thay are metal

6 0

3 years ago

2. A solution is made by adding 1.23 mol of KCl to 1000.0 g of water. Assume that the

ladessa [460]

Answer:

a. 74.55 g/mol.

b. 91.70 g.

c. 8.40%.

d. 1.23 mol/L.

Explanation:

a. Calculate the formula weight of KCl.

∵ Formula weight of KCl = atomic weight of K + atomic weight of Cl

atomic weight of K = 39.098 g/mol, atomic weight of Cl = 35.45 g/mol.

∴ Formula weight of KCl = atomic weight of K + atomic weight of Cl = 39.098 g/mol + 35.45 g/mol = 74.548 g/mol ≅ 74.55 g/mol.

b. Calculate the mass of KCl in grams.

we can use the relation:

no. of moles (n) = mass/molar mass.

∴ mass of KCl = n*molar mass = (1.23 mol)*(74.55 g/mol) = 91.69 g ≅ 91.70 g.

c. Calculate the percent by mass of KCl in this solution.

The mass % of KCl = (mass of KCl/mass of the solution) * 100.

mass of KCl = 91.70 g,

mass of the solution = 1000.0 g of water + 91.70 g of KCl = 1091.70 g.

∴ The mass % of KCl = (91.70 g/1091.70 g)*100 = 8.399% ≅ 8.40%.

d. Calculate the molarity of the solution.

Molarity is the no. of moles of solute per 1.0 L of the solution.

M = (no. of moles of KCl)/(Volume of the solution (L))

no. of moles of KCl = 1.23 mol,

Volume of the solution = mass of water / density of water = (1000.0 g)/(1.00 g/mL) = 1000.0 mL = 1.0 L.

M = (1.23 mol)/(1.0 L) = 1.23 mol/L.

3 0

4 years ago