The mass of compound is given. By using the mass, the number of phosphorous atoms present in each of the compound given in exercise 52 is to be determined. Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons. Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound. The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it. The amount of substance containing 12 g of pure carbon is called a mole. One mole of atoms always contains 6 .022 × 10 23 molecules. The number of molecules in one mole is also called Avogadro’s number . To determine : The number of phosphorous ( P ) atoms in 1 .00 g of P 4 O 6 .
The mass of compound is given. By using the mass, the number of phosphorous atoms present in each of the compound given in exercise 52 is to be determined. Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons. Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound. The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it. The amount of substance containing 12 g of pure carbon is called a mole. One mole of atoms always contains 6 .022 × 10 23 molecules. The number of molecules in one mole is also called Avogadro’s number . To determine : The number of phosphorous ( P ) atoms in 1 .00 g of P 4 O 6 .
Definition Definition Number of atoms/molecules present in one mole of any substance. Avogadro's number is a constant. Its value is 6.02214076 × 10 23 per mole.
Chapter 3, Problem 62E
(a)
Interpretation Introduction
Interpretation: The mass of compound is given. By using the mass, the number of phosphorous atoms present in each of the compound given in exercise 52 is to be determined.
Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.
Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.
The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.
The amount of substance containing
12g of pure carbon is called a mole. One mole of atoms always contains
6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.
To determine: The number of phosphorous
(P) atoms in
1.00g of
P4O6.
(a)
Expert Solution
Explanation of Solution
Given
The mass of
P4O6 is
1.00g.
The molar mass of
P4O6 is
219.866g/mol.
Formula
The number of moles in
P4O6 is calculated as,
MolesofP4O6=MassofP4O6MolarmassofP4O6
Substitute the values of mass and molar mass of
P4O6 in above equation.
The number of atoms is calculated by multiplying the number of moles with Avogadro’s number.
(b)
Interpretation Introduction
Interpretation: The mass of compound is given. By using the mass, the number of phosphorous atoms present in each of the compound given in exercise 52 is to be determined.
Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.
Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.
The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.
The amount of substance containing
12g of pure carbon is called a mole. One mole of atoms always contains
6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.
To determine: The number of phosphorous
(P) atoms in
1.00g of
Ca3(PO4)2.
(b)
Expert Solution
Explanation of Solution
Given
The mass of
Ca3(PO4)2 is
1.00g.
The molar mass of
Ca3(PO4)2 is
310.172g/mol.
Formula
The number of moles in
Ca3(PO4)2 is calculated as,
The number of atoms is calculated by multiplying the number of moles with Avogadro’s number.
(c)
Interpretation Introduction
Interpretation: The mass of compound is given. By using the mass, the number of phosphorous atoms present in each of the compound given in exercise 52 is to be determined.
Concept introduction: The atomic mass is defined as the sum of number of protons and number of neutrons.
Molar mass of a substance is defined as the mass of the substance in gram of one mole of that compound.
The molar mass of any compound can be calculated by adding of atomic weight of individual atoms present in it.
The amount of substance containing
12g of pure carbon is called a mole. One mole of atoms always contains
6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.
To determine: The number of phosphorous
(P) atoms in
1.00g of
Na2HPO4.
(c)
Expert Solution
Explanation of Solution
Given
The mass of
Na2HPO4 is
1.00g.
The molar mass of
Na2HPO4 is
141.955g/mol.
Formula
The number of moles in
Na2HPO4 is calculated as,
MolesofNa2HPO4=MassofNa2HPO4MolarmassofNa2HPO4
Substitute the values of mass and molar mass of
Na2HPO4 in above equation.
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GAY
Organic Reactions Assignment
/26
Write the type of reaction that is occurring on the line provided then complete the reaction. Only include the
major products and any byproducts (e.g. H₂O) but no minor products. Please use either full structural
diagrams or the combination method shown in the lesson. Skeletal/line diagrams will not be accepted.
H3C
1.
2.
CH3
A
Acid
OH
Type of Reaction:
NH
Type of Reaction:
+ H₂O
Catalyst
+ HBr
3.
Type of Reaction:
H3C
4.
Type Reaction:
5. H3C
CH2 + H2O
OH
+
[0]
CH3
Type of Reaction:
6. OH
CH3
HO
CH3 +
Type of Reaction:
7.
Type of Reaction:
+ [H]
humbnai
Concentration Terms[1].pdf ox + New
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Inter Concreting Concentration forms.
Hydrogen peroxide is
a powerful oxidizing agent
wed in concentrated solution in rocket fuels and
in dilute solution as a
hair bleach. An aqueous
sulation of H2O2 is 30% by mass and has
density of #liligime calculat the
Ⓒmolality
⑥mole fraction of
molarity.
20
9.
B. A sample of Commercial Concentrated hydrochloric
ET
If a reaction occurs, what would be the major products? Please include a detailed explanation as well as a drawing showing how the reaction occurs and what the final product is.