C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(I) + 2800 kJ Occasionally, not all values are found in the table of thermodynamic data. For most substances it is impossible to go into a lab and directly synthesize a compound from its free elements. The heat of formation for the substance must be calculated by working backwards from its heat of combustion. Calculate the AHf of C6H1206(s) given the combustion reaction above along with the following information. Substance AH; ° (kJ/mol) CO2(g) -393.5 H2O(1) -285.8

Trinitrotoluene (TNT) is a highly explosive compound. The thermal decomposition of TNT is described by the following chemical equation:   The enthalpy change for the explosion of ammonium nitrate with fuel oil is –7198.00 kJ for 3 moles of NH4NO3. If ΔHrxn for the thermal decomposition of 2 moles of TNT is –20,306.00 kJ, how much TNT is needed to equal the explosive power of 1 mole of ammonium nitrate?      g TNT

. Using the table provided, calculate the thermodynamic property of interest for each given reaction. Thermodynamic Data at 25 °C Species AH in kJ/mol AGº in kJ/mol So in J/(mol·K) Cu (s) 33.2 Cu (g) 337.4 297.7 166.4 CuO (s) -157.3 -129.7 42.6 H2 (g) 131.0 H2O (g) -241.8 -228.6 188.7 H2O (€) -285.8 -237.2 69.9 NO (g) 91.3 87.6 210.8 NO2 (g) 33.2 51.3 240.1 N2O4 (E) -19.5 97.5 209.2 N2O4 (g) 9.16 99.8 304.4 O2 (g) 205.0 ) Determine AS° for H2 (g) + ½ O2 (g) → H2O (g) at 25 °C. (ii) Determine AG° for 2 Cu (s) + O2 (g) → 2 CuO (s) at 25 °C. (iii) Determine AH° for H2O (8) → H2O (g) at 100 °C. (iv) Determine AG° for 2 NO2 (g) + N2O4 (g) at 100 °C.

also, Change in Gibbs Free energy Reaction Spontaneity

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H* ions; that is, AH H* (aq)]=0. H₂O HC1 (g) →H (aq) + Cl¯ (aq) Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 1 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. Part 2 of 2 □ 0x10 X □ 0.0 kJ ΔΗ% = -14.7 mol S Calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25 °C. Round your answer to 3 significant digits. 010

Estimate ΔHrxn for the following reaction: C2H4+H2→C2H6 Give your answer in kJ per mole.

The industrial synthesis of chloroform by the reaction of methane with Cl2 is carried out according to the following reaction equation:     CH4 (g)   +  Cl2 (g)   → CHCl3 (l)  +  HCl (g)   Using the thermodynamic data provided, calculate DHo (in Kj/mol) for this reaction.

Measurements show that the energy of a mixture of gaseous reactants increases by 178. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that - 143. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture | kJ during the reaction. Round your answer to 3 significant digits. x10 ? exothermic Is the reaction exothermic or endothermic? endothermic

Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 253. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 149. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 |kJ х10 significant digits. exothermic Is the reaction exothermic or endothermic? endothermic

A student dissolves 11.0 g of potassium hydroxide (KOH) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 22.0 °C to 33.7 °C over the course of 8.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: КОН(:) K*(aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. I kJ Calculate…