Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 6, Problem 6.71PAE
Interpretation Introduction
Interpretation:
Comparison between the ionization energy of oxygen and nitrogen
Concept introduction:
Ionization energy is defined as the amount of energy required to remove an electron from gaseous atom.
Ionization energy of an atom is higher in case of stable configuration state.
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Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NO(g) +Cl₂ (g) = 2NOC1 (g) AGº = -41. kJ
Now suppose a reaction vessel is filled with 8.90 atm of chlorine (C12) and 5.71 atm of nitrosyl chloride (NOC1) at 1075. °C. Answer the following questions
about this system:
rise
Under these conditions, will the pressure of NOCI tend to rise or fall?
x10
fall
Is it possible to reverse this tendency by adding NO?
In other words, if you said the pressure of NOCI will tend to rise, can that
be changed to a tendency to fall by adding NO? Similarly, if you said the
pressure of NOCI will tend to fall, can that be changed to a tendency to
rise by adding NO?
yes
no
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of NO needed to reverse it.
Round your answer to 2 significant digits.
atm
☑
18
Ar
Identifying the major species in weak acid or weak base equilibria
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that HCN is a weak acid.
acids:
0.29 mol of NaOH is added
to 1.0 L of a 1.2M HCN
solution.
bases:
☑
other:
0.09 mol of HCl is added to
acids:
1.0 L of a solution that is
bases:
0.3M in both HCN and
KCN.
other:
0,0,...
?
00.
18
Ar
日
Chapter 6 Solutions
Chemistry for Engineering Students
Ch. 6 - describe trace analysis and explain its role in...Ch. 6 - describe waves in terms of frequency, wavelength,...Ch. 6 - Prob. 3COCh. 6 - relate the frequency, wavelength, and amplitude of...Ch. 6 - describe the photoelectric effect by stating what...Ch. 6 - Prob. 6COCh. 6 - • use Planck’s equation to calculate the energy of...Ch. 6 - Prob. 8COCh. 6 - Prob. 9COCh. 6 - • describe similarities and differences between...
Ch. 6 - Prob. 11COCh. 6 - Prob. 12COCh. 6 - • identify an orbital (as 1s, 3p, etc.) from its...Ch. 6 - • list the number of orbitals of each type (1s,...Ch. 6 - • sketch the shapes of s and p orbitals and...Ch. 6 - • rank various orbitals in terms of size and...Ch. 6 - Prob. 17COCh. 6 - Prob. 18COCh. 6 - Prob. 19COCh. 6 - Prob. 20COCh. 6 - Prob. 6.1PAECh. 6 - 6.2 Unlike XRF, AAS cannot be used for...Ch. 6 - Prob. 6.3PAECh. 6 - Prob. 6.4PAECh. 6 - Prob. 6.5PAECh. 6 - Prob. 6.6PAECh. 6 - Explain why light is referred to as...Ch. 6 - Prob. 6.8PAECh. 6 - 6.7 Arrange the following regions of the...Ch. 6 - 6.8 Calculate the wavelength in meters, of...Ch. 6 - 6.9 If a string of decorative lights includes...Ch. 6 - 6.10 Define the term refraction.Ch. 6 - 6.11 Define the term photon.Ch. 6 - Prob. 6.14PAECh. 6 - 6.12 Find the energy of a photon with each of the...Ch. 6 - 6.13 Place these types of radiation in order of...Ch. 6 - 6.14 For photon with the following energies,...Ch. 6 - Prob. 6.18PAECh. 6 - 6.16 Various optical disk drives rely on laser...Ch. 6 - 6.17 The laser in most supermarket barcode...Ch. 6 - 6.18 Assume that a microwave oven operates at a...Ch. 6 - 6.19 Fill in the blanks below to complete a...Ch. 6 - 6.20 When light with a wavelength of 58.5 nm...Ch. 6 - 6.21 The electron binding energy fur copper metal...Ch. 6 - What is the difference between continuous and...Ch. 6 - Prob. 6.26PAECh. 6 - 6.23 Describe how the Bohr model of the atom...Ch. 6 - 6.24 According to the Bohr model of the atom, what...Ch. 6 - 6.25 Define the term ground state.Ch. 6 - 6.26 The figure below depicts the first four...Ch. 6 - 6.27 Refer w the data and energy-Ievel diagram...Ch. 6 - 6.28 A neon atom cmi light at many wavelengths,...Ch. 6 - 6.29 A mercury atom emits light at many...Ch. 6 - 6.30 How did the observation of electron...Ch. 6 - 6.31 Why do we use a wave function to describe...Ch. 6 - 6.32 What are the mathematical origins of quantum...Ch. 6 - Prob. 6.37PAECh. 6 - 6.34 Which of the following represent valid sets...Ch. 6 - 6.35 A particular orbital has n = 4 and l = 2....Ch. 6 - 6.36 Why are there no 2d orbitals?Ch. 6 - 6.34 What is the maximum number of electrons in an...Ch. 6 - 6.38 How many orbitals correspond to each of the...Ch. 6 - Prob. 6.43PAECh. 6 - Prob. 6.44PAECh. 6 - 6.40 Referring to Figure 6.15, draw a 4p orbitals,...Ch. 6 - Prob. 6.46PAECh. 6 - 6.43 Define the term spin paired.Ch. 6 - 6.44 On what does the Pauli exclusion principle...Ch. 6 - Prob. 6.49PAECh. 6 - Prob. 6.50PAECh. 6 - Prob. 6.51PAECh. 6 - 6.47 Depict two ways to place electrons in the 2p...Ch. 6 - 6.48 Write the ground state electron configuration...Ch. 6 - 6.49 Which of these electron configurations are...Ch. 6 - 6.50 From the list of atoms and ions given,...Ch. 6 - Prob. 6.56PAECh. 6 - Prob. 6.57PAECh. 6 - Prob. 6.58PAECh. 6 - Describe how valence electron configurations...Ch. 6 - Why is there no element to the immediate right of...Ch. 6 - Prob. 6.61PAECh. 6 - Prob. 6.62PAECh. 6 - 6.55 Explain why the s block of the periodic table...Ch. 6 - Prob. 6.64PAECh. 6 - Prob. 6.65PAECh. 6 - 6.60 Use the electron configurations of the alkali...Ch. 6 - 6.61 Using only a periodic table as a guide,...Ch. 6 - 6.62 Define the term ionization energy....Ch. 6 - 6.63 At which ionization for chlorine would you...Ch. 6 - 6.64 Arrange the following atoms in order of...Ch. 6 - Prob. 6.71PAECh. 6 - 6.66 Which element would you expect to have the...Ch. 6 - Prob. 6.73PAECh. 6 - 6.68 Indicate which species in each pair has the...Ch. 6 - 6.69 Compare the elements Na, B, Al, and C with...Ch. 6 - 6.70 Rank the following in order of decreasing...Ch. 6 - 6.71 Several excited states of the neon atom are...Ch. 6 - Prob. 6.78PAECh. 6 - Prob. 6.79PAECh. 6 - 6.92 The photoelectric effect can he used to...Ch. 6 - 6.93 A mercury atom is initially in its lowest...Ch. 6 - Prob. 6.82PAECh. 6 - 6.95 A metallic sample is known to be barium,...Ch. 6 - 6.96 When a helium atom absorbs light at 58.44 nm,...Ch. 6 - 6.97 Arrange the members of each of the following...Ch. 6 - 6.98 Arrange the following sets of anions in order...Ch. 6 - 6.99 The photoelectric effect can he used in...Ch. 6 - 6.100 Some spacecraft use ion propulsion engines....Ch. 6 - 6.101 Laser welding is a technique in which a...Ch. 6 - Prob. 6.90PAECh. 6 - 6.103 Atomic absorption spectroscopy is based on...Ch. 6 - 6.104 The red color in fireworks is the result of...Ch. 6 - 6.105 When we say that the existence of atomic...Ch. 6 - 6.106 When Bohr devised his model for the atom,...Ch. 6 - Prob. 6.95PAE
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- Identifying the major species in weak acid or weak base equilibria The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HF is a weak acid. acids: 0.2 mol of KOH is added to 1.0 L of a 0.5 M HF solution. bases: Х other: ☐ acids: 0.10 mol of HI is added to 1.0 L of a solution that is 1.4M in both HF and NaF. bases: other: ☐ 0,0,... ด ? 18 Ararrow_forwardIdentifying the major species in weak acid or weak base equilibria The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. acids: ☐ 1.8 mol of HCl is added to 1.0 L of a 1.0M NH3 bases: ☐ solution. other: ☐ 0.18 mol of HNO3 is added to 1.0 L of a solution that is 1.4M in both NH3 and NH₁Br. acids: bases: ☐ other: ☐ 0,0,... ? 000 18 Ar B 1arrow_forwardUsing reaction free energy to predict equilibrium composition Consider the following equilibrium: 2NH3 (g) = N2 (g) +3H₂ —N2 (g) AGº = 34. kJ Now suppose a reaction vessel is filled with 4.19 atm of ammonia (NH3) and 9.94 atm of nitrogen (N2) at 378. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH 3 tend to rise or fall? ☐ x10 fall Х Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH 3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no atm 00. 18 Ar 무ㅎ ?arrow_forward
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