Solution:
The solutions of the given parts are attached here.
Need help! 3. Do you expect the following reaction to be spontaneous? Why or why not-qualitatively?...
In the Check Your Learning section how did they get that value
of K?
Calculating an Equilibrium Constant using Standard Free Energy Change Given that the standard free energies of formation of Ag'(aq), CI (aq), and AgCl(s) are 77.1 kJ/mol, -131.2 kJ/mol, and -109.8 kJ/mol, respectively, calculate the solubility product, Ksp, for AgCl. Solution The reaction of interest is the following: Ag (aq) +CI (aq) Ksp [Ag ICI] AgCl(s) The standard free energy change for this reaction is first computed...
help with the following combustion reaction. shown are the
tables and answer. I am confused with the steps to get there.
2. (a) For ethanol, CH3CH2OH, AfHº = -277.7 kJ/mol at 25 °C. Using other AfHº values from Appendix A (Table 4.1) of your text, determine the enthalpy (heat) of combustion of liquid ethanol. (b) Determine the temperature change expected when 2.07 g of ethanol are burned in a bomb calorimeter whose heat capacity (as previously measured) is 9007 J/K...
#6-9
6. Calculate the enthalpy change for the reaction given below, using thermodynamic tables in your book (Appendix 2): CH(g)+02(B) HO(g) + CO,(g) (not balanced) 7. Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide: CaCO3 CO2+ CaO Using data from the textbook (Apendix 2), determine the heat of reaction. 8. When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCI+3 02 2KCIO3 Using data from the textbook (Appendix 2),...
(7 pts.) Calculate the heat absorbed when 4.20 g of H2 are produced according to the following equation. CH3OH (g) → CO(g) + 2 H2(g) AH = 90.2 kJ (7 pts.) When one adds 1.475 kJ of heat energy to a sample of gold, the temperature goes from 12.5 °C to 84.6 °C. Calculate the mass of the sample of gold. Gold has a specific heat capacity of 0.129 J/g.°C. (6 pts.) 10. Write the thermochemical equation for the standard...