Chemical Principles
8th Edition
ISBN: 9781305581982
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 13, Problem 141CP
Calculate the standard heat of formation of the compoundICl(g) at 25°C. (Hint: Use Table 13.6 and Appendix4 data.)
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16).
Using the thermochemical data below calculate the lattice energy for the formation of Na₂O.
Na(s) → Na(g)
107.3 kJ/mol
Na(g) → Na (g) + 1 e
-
495.9 kJ/mol
-418 kJ/mol
249.1 kJ/mol
-141 kJ/mol
-1484.5 kJ/mol
2 Na(s) + O₂(g) →→→ Na₂O(s)
1/2 O₂(g) → 0(g)
O(g) + 1 e→O(g)
O(g) +1e0²(g)
16) (
, Using the thermochemical data below calculate the lattice energy for the formation of Na₂O.
Na(s) → Na(g)
107.3 kJ/mol
Na(g) → Na*(g) + 1 e
495.9 kJ/mol
2 Na(s) + O₂(g) → Na₂O(s)
-418 kJ/mol
1/2 O₂(g) → O(g)
249.1 kJ/mol
O(g) + 1 e→O(g)
-141 kJ/mol
-1484.5 kJ/mol
O(g) + 1 e0²(g)
s) If 115
or pressu
26. When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200°C in a
closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established.
a) Write a balanced chemical equation for the equilibrium reaction.
b) Use bond enthalpies to estimate the enthalpy change for the reaction.
c) Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium,
the entropy effect or the energy effect?
d) In which direction will the equilibrium shift as the temperature increases above 200°C? Explain.
e) Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift?
f) Why is the equilibrium not established at room temperature?
Chapter 13 Solutions
Chemical Principles
Ch. 13 - Explain the electronegativity trends across a row...Ch. 13 - Prob. 2DQCh. 13 - Prob. 3DQCh. 13 - Prob. 4DQCh. 13 - Prob. 5DQCh. 13 - Prob. 6DQCh. 13 - Prob. 7DQCh. 13 - Prob. 8DQCh. 13 - Prob. 9DQCh. 13 - Arrange the following molecules from most to least...
Ch. 13 - Prob. 11DQCh. 13 - Prob. 12DQCh. 13 - Prob. 13ECh. 13 - Prob. 14ECh. 13 - An alternative definition of electronegativity...Ch. 13 - Prob. 16ECh. 13 - Without using Fig. 13.3, predict the order of...Ch. 13 - Without using Fig. 13.3, predict which bond in...Ch. 13 - Prob. 19ECh. 13 - Prob. 20ECh. 13 - Indicate the bond polarity (show the partial...Ch. 13 - Prob. 22ECh. 13 - Prob. 23ECh. 13 - Prob. 24ECh. 13 - Prob. 25ECh. 13 - Prob. 26ECh. 13 - Prob. 27ECh. 13 - Prob. 28ECh. 13 - Prob. 29ECh. 13 - Prob. 30ECh. 13 - Prob. 31ECh. 13 - Give an example of an ionic compound where both...Ch. 13 - What noble gas has the same electron configuration...Ch. 13 - Which of the following ions have noble gas...Ch. 13 - Give three ions that are isoelectronic with...Ch. 13 - Prob. 36ECh. 13 - Predict the empirical formulas of the ionic...Ch. 13 - Which compound in each of the following pairs of...Ch. 13 - Use the following data to estimate Hf for...Ch. 13 - Use the following data to estimate Hf for...Ch. 13 - Consider the following:...Ch. 13 - In general, the higher the charge on the ions in...Ch. 13 - Consider the following energy changes: a....Ch. 13 - Prob. 44ECh. 13 - Prob. 45ECh. 13 - The lattice energies of FeCl3,FeCl2,andFe2O3 are...Ch. 13 - Prob. 47ECh. 13 - Prob. 48ECh. 13 - Prob. 49ECh. 13 - Prob. 50ECh. 13 - Prob. 51ECh. 13 - Prob. 52ECh. 13 - Prob. 53ECh. 13 - Prob. 54ECh. 13 - Prob. 55ECh. 13 - Prob. 56ECh. 13 - Prob. 57ECh. 13 - Prob. 58ECh. 13 - Prob. 59ECh. 13 - Prob. 60ECh. 13 - Prob. 61ECh. 13 - Prob. 62ECh. 13 - Prob. 63ECh. 13 - Prob. 64ECh. 13 - Prob. 65ECh. 13 - Prob. 66ECh. 13 - Prob. 67ECh. 13 - Prob. 68ECh. 13 - Prob. 69ECh. 13 - Prob. 70ECh. 13 - Prob. 71ECh. 13 - Prob. 72ECh. 13 - Prob. 73ECh. 13 - Prob. 74ECh. 13 - Prob. 75ECh. 13 - Prob. 76ECh. 13 - Prob. 77ECh. 13 - Prob. 78ECh. 13 - Prob. 79ECh. 13 - Prob. 80ECh. 13 - Prob. 81ECh. 13 - Prob. 82ECh. 13 - Prob. 83ECh. 13 - Prob. 84ECh. 13 - Prob. 85ECh. 13 - Prob. 86ECh. 13 - Prob. 87ECh. 13 - Prob. 88ECh. 13 - Prob. 89ECh. 13 - Prob. 90ECh. 13 - Prob. 91ECh. 13 - Prob. 92ECh. 13 - Prob. 93ECh. 13 - Prob. 94ECh. 13 - Prob. 95ECh. 13 - Predict the molecular structure and the bond...Ch. 13 - Prob. 97ECh. 13 - Two variations of the octahedral geometry are...Ch. 13 - Prob. 99ECh. 13 - Predict the molecular structure and the bond...Ch. 13 - Which of the molecules in Exercise 96 have net...Ch. 13 - Prob. 102ECh. 13 - Give two requirements that should be satisfied for...Ch. 13 - What do each of the following sets of...Ch. 13 - Prob. 105ECh. 13 - Consider the following Lewis structure, where E is...Ch. 13 - Consider the following Lewis structure, where E is...Ch. 13 - Prob. 108ECh. 13 - Prob. 109ECh. 13 - Which of the following molecules have net dipole...Ch. 13 - Prob. 111AECh. 13 - Prob. 112AECh. 13 - Prob. 113AECh. 13 - Prob. 114AECh. 13 - Prob. 115AECh. 13 - There are two possible structures of XeF2Cl2 ,...Ch. 13 - Prob. 117AECh. 13 - Prob. 118AECh. 13 - Prob. 119AECh. 13 - Prob. 120AECh. 13 - Prob. 121AECh. 13 - Prob. 122AECh. 13 - Prob. 123AECh. 13 - Prob. 124AECh. 13 - Prob. 125AECh. 13 - Prob. 126AECh. 13 - Prob. 127AECh. 13 - Prob. 128AECh. 13 - Prob. 129AECh. 13 - Prob. 130AECh. 13 - Prob. 131AECh. 13 - Prob. 132AECh. 13 - Prob. 133CPCh. 13 - Prob. 134CPCh. 13 - Given the following information: Heat of...Ch. 13 - Prob. 136CPCh. 13 - A promising new material with great potential as...Ch. 13 - Think of forming an ionic compound as three steps...Ch. 13 - Prob. 139CPCh. 13 - Prob. 140CPCh. 13 - Calculate the standard heat of formation of the...Ch. 13 - Prob. 142CPCh. 13 - Prob. 143MP
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- The lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.arrow_forwardThe standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?arrow_forwardWhich statement(s) is/are true about bond enthalpy? (a) The bond energy for a triple bond between A and B is three times that of a single bond between A and B. (b) H for the breaking of a bond is always a negative number. (c) Energy is required to make a bond. (d) Bond enthalpy is defined only for bonds broken or formed in the gaseous state. (e) The presence of bonds does not influence the geometry of a molecule. However, the presence of bonds affects the value of the bond enthalpy between two atoms.arrow_forward
- Use a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.arrow_forwardGiven the following data: NO2(g) NO(g) + O(g)H = 233 kJ 2O3(g) 3O2(g)H = 427 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate the bond energy for the O2 bond, that is, calculate H for: O2(g) 2O(g)H = ?arrow_forwardWhat is the enthalpy of formation of water under standard state conditions? (See Appendix I| of your textbook.) O-241.8 kJ/mol O -237.1 kJ/mol O-285.8 kJ/mol O-228.6 kJ/molarrow_forward
- Concerning the reaction: HCN (g)-> H (g) + C (g) + N (g) which statement is flase? The reaction is known as atomization reaction. A The enthalpy of this reaction is positive. B. C. The enthalpy of this reaction is equal to the sum of enthalpies of formation the atoms: H, C, and N. The enthalpy of this reaction is equal to the sum of the bond energies of C-H and CEN. D.arrow_forwardCalculate the heat of sublimation of PI3[PI3(s)→PI3(g)]. The standard heat of formation of PI3(s) is -24.7 kJ/mol and the PI bond energy in this molecule is 184 kJ/mol. The standard heat of formation of P(g) is 334 kJ/mol and that of I2(g) is 62 kJ/mol. The I2 bond energy is 151 kJ/mol.arrow_forward(e) The mean bond enthalpy for chlorine is +242 kJ mol·l and that for fluorine is +158 kJ mol-". The enthalpy of formation of CIF (g) is 56 kJ mol·l (ii) Calculate the enthalpy of formation of, gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment. Explain.arrow_forward
- The lattice energy of an ionic compound is defined to be the amount of energy required to completely separate one mole of the solid into is gaseous ions. The lattice energy of Na2O is 2695 kJ/mol. Type the balanced chemical equation, including phase labels [ (s), (l), (g), (aq)] for the reaction that illustrates what happens when 2695 kJ of energy is added to 1 mole of solid Na2O .arrow_forwardgive an example of enthalpy change of formationarrow_forward1. Hydrogen (H2) and oxygen (O2) react to produce water (H2O). (a) Write down the equation for the above reaction. (b) The enthalpy change of reaction is –286 kJ mol-!. Is the reaction endothermic or exothermic? (c) What kinds of bonds are broken during the reaction? (d) What kinds of bonds are formed during the reaction? (e) Construct a diagram showing the change in enthalpy for the reaction.arrow_forward
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