Predict the compound in the following pair with the higher decomposition temperature. LiCO3 and NaCO3 Answer: Determine which of the statements below gives reason for your prediction: a. For the decomposition of group 1 carbonates, ArH (M₂O) becomes more endothermic down the group . Group 1 carbonates are relatively stable to heating. LiCO3 is an exception. Lit is a small positive cation with high charge density +

Predict the compound in the following pair with the higher decomposition temperature. LiCO3 and NaCO3 Answer: Determine which of the statements below gives reason for your prediction: a. For the decomposition of group 1 carbonates, ArH (M₂O) becomes more endothermic down the group . Group 1 carbonates are relatively stable to heating. LiCO3 is an exception. Lit is a small positive cation with high charge density +

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 45QAP: Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon...

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The standard enthalpy of formation of XeF4 is 218 kJ/mol. Use this value and the enthalpy of dissociation of the FF bond to calculate the XeF bond dissociation enthalpy.
Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.
The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine; ClO- is reduced to Cl-. The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, Na2S2O3; I2 is reduced to I-. The sodium thiosulfate is oxidized to sodium tetrathionate, Na2S4O6. In this analysis, potassium iodide was added in excess to 5.00 mL of bleach (d=1.00g/cm3) . If 25.00 mL of 0.0700 M Na2S2O3 was required to reduce all the iodine produced by the bleach back to iodide, what is the mass percent of NaClO in the bleach?
NaF and CaO.Which has the higher melting point and why?
What is the enthalpy change, Delta Hrxn, for the following reaction? 2 NaOH (s) + CO2 (g) → Na2CO3 (s) + H2O (l) a. – 597.5 kJ b. – 991.0 kJ c. + 171.9 kJ d. none of these e. +2661.4 kJ f. – 2661.4 kJ g. – 171.9 kJ h. + 991.0 kJ
18. Name two ions associated with Group 1 cations, and explain what is the difference between Group 1 cations, and how do they differ from Group 4 cations? Give examples. 19. How can PbCl2 be separated from AgCl and Hg2Cl2
At 400 °C, the AG an for the oxidation of a monoatomic liquid element Z in the presence of 02(g) forming ZO) is -25.0 kJ per mol O2. In the compound ZOs, Z has a +2 formal charge. Which of the following statements is CORRECT? The oxidation of Z with O2 is marked by an increase in entropy. O Z cannot be oxidized to Z0 because Z is more stable than ZO at 400 °C or any T above it. O The oxidation of Z with 02 is exothermic, O zo cannot be reduced back to Z at any temperature because reduction of ZO to Z has +AG.
The breaking of the O-O bond in peroxydisulfuryl difluoride (FO,SOOSO,F) gives FO,SO: (FO2SO)2 2 2 FO2SO The compound on the left of this equation is a colorless liquid that boils at 67.1°C. Its vapor, when heated to about 100°C, turns brown as the product of the reaction forms. Suppose that, in a sample of the vapor, the intensity of the brown color doubles between 100°C and 110°C and that the total pressure increases only by the 2.7% predicted for an ideal gas. Estimate AH° for the preceding reaction.
4. The common oxidation number for an alkaline earth metal is +2. (a) Using the Born-Mayer equation (for determining the lattice enthalpy) and a Born-Haber cycle (draw it), show that CaCl is an exothermic compound (negative AHf). Make a reasonable prediction to estimate the ionic radius of Ca (explain your reasoning). The sublimation (atomization) enthalpy for Ca(s) is 178 kJ/mol. (b) Show that an explanation for the non-existence of CaCl can be found in the enthalpy change for the reaction below. The AHf for CaCl2(s) is -190.2 kcal/mol. 2 CaCl(s) → Ca(s) + CaCl2(s)
Using the thermodynamic tables find the enthalpy of formation for BaCO3 (s). a. + 314.4 kJ b. – 1219 kJ c. – 628.8 kJ d. – 1.29 x 103 kJ e. – 5.16 x 103 kJ f. none of these g. – 314.4 kJ
Using the thermodynamic tables find the enthalpy of formation for BaCO3 (s). a. – 1.29 x 103 kJ b. – 5.16 x 103 kJ c. – 628.8 kJ d. – 1219 kJ e. + 314.4 kJ f. – 314.4 kJ g. none of these
An instant cold pack purchased in a pharmacy contains a packet of solid ammonium nitrate surrounded by a pouch of water. When the packet of NH4NO3 is broken, the solid dissolves in water and cooling of the mixture occurs because the solution process for NH4NO3 is endothermic. Explain, in terms of what happens to the molecules and ions, why this mixing occurs spontaneously. Select all that apply. In solution, the ions NH4* and NO3 are highly ordered throughout the solvent. In the solid, the ions in NH4NO3 are highly ordered. In solution, the ions NH4+ and NO3 are randomly distributed throughout the solvent. The increase in randomness makes the process spontaneous. The decrease in randomness makes the process spontaneous.