Heat capacity data can be used to estimate the reaction enthalpy at one temperature from its value at another. Predict the standard reaction enthalpy of 2 NO2(g) → N2O4 (g) at 100 °C from its value at 25 °C.

Given, Salt: FeCl2 Mass of salt: 4.843  Mass of water: 45.1  Initial temp: 20.00  Final Temp: 32.663239    The sample of this salt is placed in water at a constant pressure calorimeter with a heat capacity of 35.5 J/℃.  Determine the enthalpy change for the dissociation of this salt, ΔHdiss.  1.    Σ qi  =  qreaction + qsolution + qcalorimeter =  0              Calculate the heat of the solution.      2. Calculate the heat of the calorimeter.   3. Calculate the heat of the reaction.   4. How many moles of your salt dissolved?   5. Calculate the value of ΔHdiss.

For the combustion of 1.00 mol of toluene, C7H8 , at 25 °C and 1.00 bar, calculate the work that must be done against the atmosphere for the expansion of the gaseous products. ?=   Using the enthalpy of formation data, calculate the standard enthalpy of reaction, Δ?° . Δ?°=   Calculate the change in internal energy, Δ?° , of the system. Δ?°=

Find the molar enthalpy of combustion in kJ/mol of glucose at some temperature and pressure C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) given that in an experiment under the same conditions the combustion of 0.108 g of glucose raised the temperature of a calorimeter with total heat capacity C= 1.155 kJ/°C by 1.31 °C. The molar mass of glucose is 180.1 g/mol. Ignore the heat absorbed by the combustion products; assume this is negligible, and all heat went into the calorimeter itself. Give the answer with 5 or more significant figures.

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

Determine the enthalpy change for the reaction: S03 (g) + H20(g) → H2SO4 (1) Given: i. H2SO4 (1) → H2SG) + 2 02 (9); ΔΗ 1236.4 kJ %3D ii. SO3 + H20(1) H2S(9) + 2 02 (9); ΔΗ1086.7 ky (g) iii. H20(1) → H20(g); AH° = 40.7 kJ

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

PCI5(s) can be prepared by the reaction PCI3(1) + Cl2(g) - PCI5(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCI5(s) by the above reaction, given the following data. P4(s) + 6 Cl2(g) - 4 PC|3(1) AH° = -1280 kJ per mole of P4(s) %3D P4(s) + 10 Cl2(g) – 4 PCI5(s) ΔΗ AH° = -1774 kJ per mole of P4(s) +59.3 -59.3 +124 -124 -258

using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or 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