What are the uses of evaporative salts?
Answers
Answer : Evaporative salts are majorly used as common salts or halites, which are highly and widely used to preserve foods, dye fabric, and de-ice roads.
Explanation : Evaporative salts are produced by evaporation of the sea water hence it is named as evaporative salts. These are mainly extracted through evaporation from seawater. The salts from shallow ponds where the seawater gets collected in a land, which is later harvested and then purified.
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Compared to the energy and charge of the electrons in the first shell of a Be atom, the electrons in the second shell of this atom have
Salt water is classified as a1) compound because the proportion of its atoms is fixed2) compound because the proportion of its atoms can vary3) mixture because the proportion of its components is fixed4) mixture because the proportion of its components can vary
How many grams of KOH used to make 1.6 liters of 15% by mass solution with water as the solvent?
A mixture of sand and salt containig MgCl2 (100.0 g) is sprinkled on a section of pavement. The total estimated ice on the pavement is 10.0 kg. What is the freezing point of the ice (°C)? MM MgCl2 = 95.211 g/mol MM ice = 18.0148 g/mol
16 H+ (aq) + 2 Cr2O7 2-(aq) + C2H5OH (aq) ? 4 Cr3+ (aq) + 2 CO2 (g) + 11 H2O (l)
If 35.46 mL of 0.05961 M Cr2O7 2-
is required to titrate 28.00 g of plasma, what is the mass percent
of alcohol in the blood?
Answers
Answer:
0.17%
Explanation:
With the equation:
2Cr2O7 2- + C2H5OH + H2O --> 4Cr3+ + 2CO2 + 11H2O
We can assume that every mole of ethanol needs 2 moles of Dichromate to react.
So if in 1L we have 0.05961 moles of dichromate we can discover how many moles we have in 35.46mL
1000 mL - 0.05962 moles
35.46 mL - x
x =
x = 2,11* 10^-3 moles
As we said earlier, 1 mole of ethanol needs 2 mole of dichromate, so in the solution we have 1,055*10^-3 moles of ethanol. We can discover the mass of ethanol present in the solution.
1 mole - 46g
1.055*10^-3 - y
y = 46 * 1.055*10^-3
y = 0.048 g
To discover the percent of alchol we can use a simple relation
28 g - 100%
0.048 - z
z =
z = 0.17%
b. solid to gas
c. liquid to gas
d. solid to liquid
Answers
Answer:
its D
Explanation:
Answers
So we are going to take our known value of 4 moles, and multiply by 6.02 x 10^23 (Avogadro's number) and we will get the number of atoms that are in 4 moles.
(4.0 moles of Na) x (6.02 x 10^23) / (1 mole) = 2.4 x 10^24 atoms of Na
There are 2.4 x 10^24 atoms of Na in 4.0 moles.
Final answer:
To find the number of atoms in 4.0 Mol of sodium, you need to multiply the number of moles by Avogadro's number. This will give you approximately 2.4088 x 10^24 atoms.
Explanation:
To calculate the number of atoms in 4.0 Mol of sodium, you need to use Avogadro's number, which is 6.022 x 1023 atoms per mole. The calculation is as follows:
Start with the number of moles given, which is 4.0 mol.Multiply this by Avogadro's number (6.022 x 1023) to get the total number of atoms:4.0 mol x 6.022 x 1023 atoms/mol = 2.4088 x 1024 atoms
So, there would be approximately 2.4088 x 1024 atoms in 4.0 mol of sodium.
Learn more about Avogadro's number here:
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Answers
Answers
Answer:approximately 115.33 grams of H2O are needed to react with 3.20 moles of CaC2 in the given reaction.
Explanation:To determine how many grams of H2O are needed to react with 3.20 moles of CaC2 in the given reaction, we can use stoichiometry and the molar ratios between CaC2 and H2O in the balanced chemical equation.
First, let's write down the balanced chemical equation:
CaC2 (s) + 2H2O (l) -> C2H2 (g) + Ca(OH)2 (aq)
From the balanced equation, we can see that 1 mole of CaC2 reacts with 2 moles of H2O.
Now, let's use this information to calculate the moles of H2O required to react with 3.20 moles of CaC2:
Moles of H2O = (3.20 moles CaC2) * (2 moles H2O / 1 mole CaC2)
Moles of H2O = 3.20 moles * 2
Moles of H2O = 6.40 moles
Now that we know we need 6.40 moles of H2O, we can calculate the grams of H2O needed using the molar mass of H2O:
Molar mass of H2O = 2(1.01 g/mol) + 16.00 g/mol = 2.02 g/mol + 16.00 g/mol = 18.02 g/mol
Now, calculate the grams of H2O:
Grams of H2O = (6.40 moles) * (18.02 g/mol)
Grams of H2O ≈ 115.33 grams
So, approximately 115.33 grams of H2O are needed to react with 3.20 moles of CaC2 in the given reaction.
Answers
Answer:
Explanation:
A pure substance is a substance that consists of only one type of particle, either atoms, molecules, or ions, and has a consistent and uniform composition throughout. Pure substances cannot be separated into other substances by physical means. They have well-defined chemical properties and distinct physical properties, such as melting point and boiling point.
Two examples of pure substances are:
Elemental Hydrogen (H2): Elemental hydrogen consists of diatomic molecules, each containing two hydrogen atoms bonded together. It is a pure substance because it consists only of hydrogen molecules and cannot be separated into other substances without chemical reactions.
Water (H2O): Water is a pure substance composed of water molecules, each consisting of two hydrogen atoms and one oxygen atom bonded together. It is also a pure substance because it has a consistent and uniform composition throughout and cannot be separated into other substances without breaking its molecular bonds.
These examples illustrate the concept of pure substances, where the composition is homogeneous and consistent throughout the entire sample.