Write equations similar to Equations 9.48 and 9.49 of the text to illustrate how a mixture of sodium hydrogen phosphate
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Chemistry for Today: General, Organic, and Biochemistry
- Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward1. Galium (Ga) is an element in group III with atomic number 31. By referring to the Periodic Table, answer the following questions. i. Explain how the atomic radius of gallium differs from aluminium. ii. Explain how the electronegativity of gallium differs from aluminium. iii. Explain how the electronegativity of gallium differs from germanium. iv. Explain how the ionisation energy of gallium differs from germanium. v. Explain how the ionisation energy of gallium differs from indium.arrow_forwardThe reaction of a metal, M, with a halogen, X2, proceeds by an exothermic reaction as indicated by this equation: M(s) + X2(g) ⟶ MX2(s). For each of the following, indicate which option will make the reaction moreexothermic. Explain your answers.(a) a large radius vs. a small radius for M+2(b) a high ionization energy vs. a low ionization energy for M(c) an increasing bond energy for the halogen(d) a decreasing electron affinity for the halogen(e) an increasing size of the anion formed by the halogenarrow_forward
- Write an equation to show that hypochlorous acid , HClO , behaves as an acid in water. + H2O = +arrow_forwardHow does the acidity of the binary acid of an element vary as a function of the electronegativity of the element? How does this relate to the position of the element in the periodic table?arrow_forwardWhy is it that Xe, a noble gas element we normally think of as being unreactive can form covalent compounds?arrow_forward
- group A solutions: Conductivity (ms) concentration of chloride ions: NaCl 6594 0.19 CaCl2 13188 0.6 AlCl3 16311 0.9 Why do the Group A compounds, each with the same concentration (0.05 M), have such large differences in conductivity values?arrow_forwardWhat is the correct Lewis structure for hydrazoic acid (HN3) including the formal changes if any ?arrow_forwardWhich on the three delta H’s was the largest? Explain why.arrow_forward
- The precious gem ruby aluminum oxide, Al2O3 containing traces of Cr3+. The compound Al2Se3 is used in the fabrication of some semiconductor devices. Which of the two has a larger lattice energy?arrow_forwardEthanol can be made by the reaction of ethylene and water: H2C=CH2(g) + H2O(g) CH3CH2OH(g) Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Compare the value obtained to the value calculated from enthalpies of formation.arrow_forwardThe equation for the combustion of gaseous methanol is 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) (a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of one mole of gaseous methanol? (b) Compare your answer in part (a) with the value of tHcalculated using enthalpies of formation data.arrow_forward
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