Use the thermodynamic quantities given below to calculate the theoretical ΔH for this reaction:       NH3 + HCl → NH4Cl ΔH°f for NH3 (aq) = - 80.29 kJ/mol ΔH°f for HCl (aq) = - 167.2 kJ/mol ΔH°f for NH4+ (aq) = - 132.5 kJ/mol ΔH°f for Cl- (aq) = - 167.2 kJ/mol I found this answer to be -52.21 kJ/mol 6. What is the percent error of experimental results when using the theoretical value calculated in Question 5? I need help finding this

Given the standard enthalpy changes for the following two reactions:(1) N2(g) + 2O2(g) -> 2NO2(g)...... ΔH° = 66.4 kJ(2) 2N2O(g) -> 2N2(g) + O2(g)......ΔH° = -164.2 kJwhat is the standard enthalpy change for the reaction:(3) 2N2O(g) + 3O2(g) -> 4NO2(g)......ΔH° = ?_____ kJ

How do I determine and write out products of this reaction? Also is this a decomposition reaction? NaHCO3 (s) →

The enthalpy for the formation of 1 mole of NH3(aq)NH3(aq) is -80.29 kJ/molkJ/mol. What is the enthapy for the formation of 3 moles of NH3(aq)NH3(aq)?

Given the overall reaction from the previous problem: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes: Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic? Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction.  If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?

Calculate the enthalpy of reaction for the following reaction: Fe₂O3(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) AH,(Fe₂O3(s)) = -824.2 kJ/mol AH(CO(g)) = -110.5 AH,(Fe(s)) = ? AH(CO₂(g)) = -393.5 kJ/mol Answer: How much energy in kJ is required to heat a calorimeter whose heat capacity is 113.4 J/°C from 23.5°C to 55.0°C?

Given the heat of formation of the following compounds:                 CO2(g)                ΔfH° = -393.5 kJ/mol                 H2O(l)                 ΔfH° = -285.9 kJ/mol                 CH3OH(l)          ΔfH° = -238.6 kJ/mol   What is the value of ΔrH° for the reaction:                 CH3OH(l) + 3/2 O2(g) → CO2(g) + 2 H2O(l)

Are the reactions endothermic or exothermic? What observation supports this?

An experiment was conducted to find the heat of neutralisation in an acid - basereaction.A solution was made by dissolving 3.79g of barium hydroxide in 100 mL of water. 30.0 mL of this barium hydroxide solution was reacted with 27.0 mL of a 0.400 mol L-1solution of nitric acid. The heat of neutralisation was calculated to be 51.7 kJ mol-1. Calculate the temperature change and the resultant pH of the solution

25.00 mL of 0.4600 M phosphoric acid are reacted with 94.00 mL of 0.7970 M sodium hydroxide. The sodium hydroxide is in excess. Initially, both solutions are at room temperature, 24.692°C. After the reaction is complete, the temperature of the solution has increased to 30.347°C. What is the enthalpy of the reaction in kJ/mol acid? Assume the density of the solution is 1.00g/mL and the specific heat of the solution is the same as water (4.184 J/g-K).