The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 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 substance always contains 6 .022 × 10 23 atoms. Hence, ( 6 .022 × 10 23 atoms ) ( 12 u 1 atom ) = 12 g ⇒ 1 u = 1 6 .022 × 10 23 g To determine : The mass of nitrogen ( N ) in 5 .00 moles of NH 3 .
The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 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 substance always contains 6 .022 × 10 23 atoms. Hence, ( 6 .022 × 10 23 atoms ) ( 12 u 1 atom ) = 12 g ⇒ 1 u = 1 6 .022 × 10 23 g To determine : The mass of nitrogen ( N ) in 5 .00 moles of NH 3 .
Solution Summary: The author explains that the number of moles of a compound is given and the mass of nitrogen in each compound given in exercise 51 is determined.
Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 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 substance always contains
6.022×1023 atoms.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The mass of nitrogen
(N) in
5.00 moles of
NH3.
(b)
Interpretation Introduction
Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 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 substance always contains
6.022×1023 atoms.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The mass of nitrogen
(N) in
5.00 moles of
N2H4.
(c)
Interpretation Introduction
Interpretation: The number of moles of compound is given. By using the number of moles, the mass of nitrogen in each compound given in exercise 51 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 substance always contains
6.022×1023 atoms.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The mass of nitrogen
(N) in
5.00 moles of
(NH4)2Cr2O7.
Recognizing ampli
Draw an a amino acid with a methyl (-CH3) side chain.
Explanation
Check
Click and drag to start drawing a
structure.
X
C
Write the systematic name of each organic molecule:
structure
name
×
HO
OH
☐
OH
CI
CI
O
CI
OH
OH
く
Check the box under each a amino acid.
If there are no a amino acids at all, check the "none of them" box under the table.
Note for advanced students: don't assume every amino acid shown must be found in nature.
COO
H3N-C-H
CH2
HO
CH3
NH3 O
CH3-CH
CH2
OH
Onone of them
Explanation
Check
+
H3N
O
0.
O
OH
+
NH3
CH2
CH3-CH
H2N C-COOH
H
O
HIC
+
C=O
H3N-C-O
CH3- - CH
CH2
OH
Х
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Chapter 5 Solutions
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