The mass of compound is given. By using the mass, the number of molecules present of each of the 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 atoms always contains 6 .022 × 10 23 molecules. The number of molecules in one mole is also called Avogadro’s number . Hence, ( 6 .022 × 10 23 atoms ) ( 12 u 1 atom ) = 12 g ⇒ 1 u = 1 6 .022 × 10 23 g To determine : The number of molecules in 1 .00 g of NH 3 .
The mass of compound is given. By using the mass, the number of molecules present of each of the 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 atoms always contains 6 .022 × 10 23 molecules. The number of molecules in one mole is also called Avogadro’s number . Hence, ( 6 .022 × 10 23 atoms ) ( 12 u 1 atom ) = 12 g ⇒ 1 u = 1 6 .022 × 10 23 g To determine : The number of molecules in 1 .00 g of NH 3 .
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 5, Problem 59E
(a)
Interpretation Introduction
Interpretation: The mass of compound is given. By using the mass, the number of molecules present of each of the 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 atoms always contains
6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The number of molecules in
1.00g of
NH3.
(a)
Expert Solution
Explanation of Solution
Given
The mass of
NH3 is
1.00g.
The molar mass of
NH3 is,
(14.006+3×1.0079)g/mol=17.0297g/mol
Formula
The number of moles in
NH3 is calculated as,
MolesofNH3=MassofNH3MolarmassofNH3
Substitute the values of mass and molar mass of
NH3 in above equation.
The number of molecules 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 molecules present of each of the 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 atoms always contains
6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The number of molecules in
1.00g of
N2H4.
(b)
Expert Solution
Explanation of Solution
Given
The mass of
N2H4 is
1.00g.
The molar mass of
N2H4 is,
(2×14.006+4×1.0079)g/mol=32.0436g/mol
Formula
The number of moles in
N2H4 is calculated as,
MolesofN2H4=MassofN2H4MolarmassofN2H4
Substitute the values of mass and molar mass of
N2H4 in above equation.
The number of molecules 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 molecules present of each of the 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 atoms always contains
6.022×1023 molecules. The number of molecules in one mole is also called Avogadro’s number.
Hence,
(6.022×1023atoms)(12u1atom)=12g⇒1u=16.022×1023g
To determine: The number of molecules in
1.00g of
(NH4)2Cr2O7.
A block of zinc has an initial temperature of 94.2 degrees celcius and is immererd in 105 g of water at 21.90 degrees celcius. At thermal equilibrium, the final temperature is 25.20 degrees celcius. What is the mass of the zinc block? Cs(Zn) = 0.390 J/gxdegrees celcius Cs(H2O) = 4.18 J/gx degrees celcus
Potential Energy (kJ)
1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction.
AH = -950 kJ
AH = 575 kJ
(i) Cl₂ (g) + Pt (s) 2C1 (g) + Pt (s)
Ea = 1550 kJ
(ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s)
(iii) Cl (g) + CICO (g) → Cl₂CO (g)
Ea = 2240 kJ
Ea = 2350 kJ
AH = -825 kJ
2600
2400
2200
2000
1800
1600
1400
1200
1000
a. Draw the potential energy diagram for the reaction. Label the data points for clarity.
The potential energy of the reactants is 600 kJ
800
600
400
200
0
-200-
-400
-600-
-800-
Reaction Progress
Can u help me figure out the reaction mechanisms for these, idk where to even start
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