Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 7, Problem 7.86PAE
7.86 Nitrogen triiodide,
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Which one of these processes corresponds to the lattice energy of NaCl(s)?
O NaCI(s) → Na*(g) + CI (g)
O Na(s) + ½ Cl2(g) NaCl(s)
O Na*(g) + CI(g) → NaCl(s)
O NaCl(s) → Na(s) + ½ Cl2(g)
The combustion of propane gas (C3H8; molar mass = 44.09 g/mol) occurs according to the following equation:
C3H8(g) + 5O2(g) --> 3CO2(g) + 4H2O(g)
Given the following standard molar enthalpy of formation (DHof), how much energy in kilojoules is produced when 1.00 g of propane is completely combusted?
DHof[C3H8] = -103.8 kJ/mol; DHof[CO2] = -393.5 kJ/mol, and DHof[H2O(g)] = -241.8 kJ/mol
(A) 2043.9 kJ
(B) 531.5 kJ
(C) 12.1 kJ
(D) 46.4 kJ
An experiment was conducted to determine the Cl - Cl bond energy in chlorine. It was determined the minimum energy required to break a Cl - Cl bond was 3.90 x 10-19 J. According to these experimental results, what is the Cl - Cl bond energy (in kJ/mol)?
Chapter 7 Solutions
Chemistry for Engineering Students
Ch. 7 - List some factors influencing the biocompatibility...Ch. 7 - • use electron configurations to explain why...Ch. 7 - • describe die energy changes in the formation of...Ch. 7 - • define electronegativity and state how...Ch. 7 - • identify or predict polar, nonpolar, and ionic...Ch. 7 - • write Lewis electron structures for molecules or...Ch. 7 - • describe chemical bonding using a model based on...Ch. 7 - • explain how hybridization reconciles observed...Ch. 7 - • predict the geometry of a molecule from its,...Ch. 7 - • use models (real or software) to help visualize...
Ch. 7 - • explain the formation of multiple bonds in terms...Ch. 7 - • identify sigma and pi bonds in a molecule and...Ch. 7 - Define the term biocompatibility.Ch. 7 - List some properties associated with biomaterials...Ch. 7 - Prob. 7.3PAECh. 7 - Prob. 7.4PAECh. 7 - Prob. 7.5PAECh. 7 - Prob. 7.6PAECh. 7 - Why is the ion not found in nature?Ch. 7 - Why do nonmetals tend to form anions rather than...Ch. 7 - Prob. 7.9PAECh. 7 - 7.10 Arrange the members of each of the following...Ch. 7 - 7.11 Arrange the following sets of anions in order...Ch. 7 - 7.12 Which pair will form a compound with the...Ch. 7 - 7.13 Figure 7-2 depicts the interactions of an ion...Ch. 7 - 7.14 Describe the difference between a covalent...Ch. 7 - 7.15 Covalently bonded compounds tend to have much...Ch. 7 - Prob. 7.16PAECh. 7 - 7.17 Coulombic forces are often used to explain...Ch. 7 - 7.18 In terms of the strengths of the covalent...Ch. 7 - 7.19 If the formation of chemical bonds always...Ch. 7 - 7.20 Draw the Lewis dot symbol for each of the...Ch. 7 - 7.21 Theoretical models for the structure of...Ch. 7 - 7.22 Use Lewis dot symbols to explain why chlorine...Ch. 7 - 7.23 Define the term lone pair.Ch. 7 - 7.24 How many electrons are shared between two...Ch. 7 - 7.25 How does the bond energy of a double bond...Ch. 7 - 7.26 How is electronegativity defined?Ch. 7 - 7.27 Distinguish between electron affinity and...Ch. 7 - 7.28 Certain elements in the periodic table shown...Ch. 7 - 7.29 When two atoms with different...Ch. 7 - 7.30 The bond in HF is said to be polar, with the...Ch. 7 - 7.31 Why is a bond between two atoms with...Ch. 7 - Prob. 7.32PAECh. 7 - 7.33 In each group of three bonds, which bond is...Ch. 7 - Prob. 7.34PAECh. 7 - 7.35 Which one of the following contains botb...Ch. 7 - Prob. 7.36PAECh. 7 - 7.37 Draw the Lewis structure for each of the...Ch. 7 - 7.38 Draw a Lewis structure for each of the...Ch. 7 - Prob. 7.39PAECh. 7 - 7.40 Why is it impossible for hydrogen to be the...Ch. 7 - Prob. 7.41PAECh. 7 - 7.42 Draw resonance structure for (a) (b) and (c)Ch. 7 - Prob. 7.43PAECh. 7 - Prob. 7.44PAECh. 7 - Prob. 7.45PAECh. 7 - 7.46 Consider the nitrogen-oxygen bond lengths in...Ch. 7 - 7.47 Which of the species listed has a Lewis...Ch. 7 - 7.48 Identify what is incorrect in the Lewis...Ch. 7 - 7.49 Identify what is incorrect in the Lewis...Ch. 7 - 7.50 Chemical species are said to be isoelectronic...Ch. 7 - 7.51 Explain the concept of wave interference in...Ch. 7 - 7.52 How does orbital overlap explain the buildup...Ch. 7 - 7.53 How do sigma and pi bonds differ? How are...Ch. 7 - 7.54 CO , CO2 , CH3OH , and CO32 , all contain...Ch. 7 - 7.55 Draw the Lewis dot structure of the following...Ch. 7 - 7.56 Draw the Lewis dot structures of the...Ch. 7 - 7.57 What observation about molecules compels us...Ch. 7 - Prob. 7.58PAECh. 7 - 7.59 What type of hybrid orbital is generated by...Ch. 7 - 7.60 What type of hybridization would be expected...Ch. 7 - 7.61 What hybrid orbitals would be expected for...Ch. 7 - 7.62 What type of hybridization would you expect...Ch. 7 - 7.63 What physical concept forms the premise of...Ch. 7 - 7.64 Predict the geometry of the following...Ch. 7 - Prob. 7.65PAECh. 7 - Prob. 7.66PAECh. 7 - Prob. 7.67PAECh. 7 - 7.68 Give approximate values for the indicated...Ch. 7 - 7.69 Propene has the chemical formula Describe the...Ch. 7 - Prob. 7.70PAECh. 7 - Prob. 7.71PAECh. 7 - 7.72 How does an MSN differ from amorphous silica...Ch. 7 - Prob. 7.73PAECh. 7 - 7.74 In a lattice, a positive ion is often...Ch. 7 - 7.75 Use the concept of lattice energy to...Ch. 7 - Prob. 7.76PAECh. 7 - Prob. 7.77PAECh. 7 - Prob. 7.78PAECh. 7 - Prob. 7.79PAECh. 7 - Prob. 7.80PAECh. 7 - Prob. 7.81PAECh. 7 - Prob. 7.82PAECh. 7 - Prob. 7.83PAECh. 7 - 7.84 Which of the following molecules is least...Ch. 7 - 7.85 Consider the molecule whose structure is...Ch. 7 - 7.86 Nitrogen triiodide, NI3(s) , is unstable and...Ch. 7 - 7.87 Nitrogen is capable of forming single,...Ch. 7 - 7.88 The N5+ cation has been synthesized and...Ch. 7 - Prob. 7.89PAECh. 7 - Prob. 7.90PAECh. 7 - 7.91 A Lewis structure for the oxalate ion is...Ch. 7 - Prob. 7.92PAECh. 7 - 7.93 An unknown metal M forms a chloride with the...Ch. 7 - Prob. 7.94PAECh. 7 - Prob. 7.95PAECh. 7 - 7.96 Consider the hydrocarbons whose structures...Ch. 7 - 7.97 Consider the structure shown below for as...Ch. 7 - Prob. 7.98PAECh. 7 - Prob. 7.99PAECh. 7 - Prob. 7.100PAECh. 7 - 7.101 Lead selenide nanocrystals may provide a...Ch. 7 - Prob. 7.102PAECh. 7 - Prob. 7.103PAECh. 7 - 7.104 Hydrogen azide, HN3 , is a liquid that...Ch. 7 - Prob. 7.105PAECh. 7 - Prob. 7.106PAECh. 7 - 7.107 How do the Lewis symbols for C, Si, and Ge...Ch. 7 - Prob. 7.108PAECh. 7 - Prob. 7.109PAE
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- A commercial process for preparing ethanol (ethyl alcohol), C2H5OH, consists of passing ethylene gas. C2H4, and steam over an acid catalyst (to speed up the reaction). The gas-phase reaction is Use bond enthalpies (Table 9.5) to estimate the enthalpy change for this reaction when 37.0 g of ethyl alcohol is produced.arrow_forwardExplain the decomposition of nitroglycerin in terms of relative bond enthalpies.arrow_forwardhat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?arrow_forward
- NaCl has a lattice energy of -787 kJ/mol. Consider a hypothetical salt XY. X3 + has the same radius of Na+ and Y3 - has the same radius as Cl - . Estimate the lattice energy of XY.arrow_forwarda) In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ Calculate the amount of energy released when one mole of hydrogen gas reacts. Consider this to be a positive value. b) How much energy is released when 20.00 g of NH3(g) is made to react with an excess of steam to form HNO3 and H2 gases? Again, enter this as a positive value. HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJarrow_forwardHess's Law is a useful way for chemists to predict the enthalpy change for a reaction. Use your understanding of energy changes to explain how Hess's Law works. Use the following example as part of your explanation (but you don't have to solve it!). 8. How can Hess's law be applied to determine the enthalpy change for the decomposition of potassium bicarbonate: 2 KHCO, (9) – K,CO; (s) + H,O () + CO2 (2) AH = -963 kJ (1) K (9) + ½ H, (e) Ce +0, (9)→ KHCO; (5) 2 (g) AH = -1150 kJ (2) 2K (9) + C + 02 (e) → K,C03 (6) AH = -242 kJ (3) H2() + ½ O2() H,O (g) AH = -394 kJ (4) C (6)+02 (g) - CO2 (2)arrow_forward
- 20. The formation of lithium fluoride, LiF, involves the following reaction: Li(s) + ½ F2(g) → LiF(s); AH= -616.0 kJ Draw the Born-Haber Cycle for the formation of lithium fluoride from lithium and fluorine gas that includes all the steps listed below, and calculate the lattice energy (UL) of LiF. Steps: AH in kJ/mol (1) Li(s) → Li(g); (2) Li(g) → Li"(g) + e"; AH, = 161; IE = 520; (3) F2(g) → 2F(g): BE = 160; (4) F(g) + e → F (g); EA = -328; Chem 1A, Midterm Exam Review#2 (5) Li"(g) + F(g) → LiF(s); UL = ? (lattice energy)arrow_forwardCyanamide is a compound containing two hydrogen atoms and some amount of C and N. There are a total of 5 atoms in the compound. The products of combustion were found to be CO2, NO2, and H2O. If the enthalpy of combustion for cyanamide is – 671.9 kJ/mol and the enthalpy of formation is 58.8 kJ/mol, what is the chemical formula for cyanamide? ( ΔfH (CO2) = - 393.51 kJ/mole; ΔfH (NO2) = + 33.10 kJ/mole; ΔfH (H2O) = - 241.826 kJ/mole)arrow_forwardCalculate the amount of energy required or released in the formation reaction for 15 moles of gaseous HI. Express your answer in joules. The heat of formation of HI is +25.9 kJ/mol. Is this an endothermic or exothermic reaction? Explain your reasoning and show all your work to receive full credit. Use the paperclip button below to attach files. XD眉 B IU MacBo II |arrow_forward
- Reaction between methane and chlorine is:CH4(g) + 2Cl2(g) → CCl4(l) + 2H2(g)and given ; ΔHf ̊ CCl4 (l) = –128.4 kJ/mol, ΔHf ̊ CH4(g) = -75kJ/molCalculate the enthalpy change for the reaction. Sketch the energy profile diagramfor the reaction.arrow_forwardWhich of the following statements about the bonds is the most correct given the reaction shown below? AH = +91 kJ/molxn CH₂OH(g) → CO(g) + 2 H₂(g) A The sum of the bond energies in the reactants is greater than the sum of the bond energies in the products B The sum of the bond energies in the reactants is less than the sum of the bond energies in the products. It is not possible to tell which bond energies are greater since the bond energies are not given. D The reaction is exothermicarrow_forwardA scientist studies the bond energies of different compounds containing nitrogen (N). The scientist observes that the N–N bonds in one group of compounds have a bond energy of 209 kJ/mol, while the N–N bonds in another group of compounds have a bond energy of 418 kJ/mol. In one or two sentences, postulate a reason for this difference.arrow_forward
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