Calculate the standard enthalpy change for the precipitation reaction between aqueous silver nitrate (AgNO3) and aqueous sodium chloride (NaCl) to form solid silver chloride (AgCl) and aqueous sodium nitrate (NaNO3), given the following balanced chemical equation:AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq) Assume that the reaction takes place under standard conditions (25°C and 1 atm) and that all solutions are at 1 M concentration.

Question

Calculate the standard enthalpy change for the precipitation reaction between aqueous silver nitrate (AgNO3) and aqueous sodium chloride (NaCl) to form solid silver chloride (AgCl) and aqueous sodium nitrate (NaNO3), given the following balanced chemical equation:AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq) Assume that the reaction takes place under standard conditions (25°C and 1 atm) a

Answer 1

To calculate the standard enthalpy change  H  for the precipitation reaction, we need to use the standard enthalpies of formation  Hf  of the reactants and products. The equation to calculate H is:H =  Hf products  -  Hf reactants The standard enthalpies of formation for the compounds involved in the reaction are as follows:Hf AgNO3  aq   = -124.4 kJ/molHf NaCl  aq   = -407.3 kJ/molHf AgCl  s   = -127.0 kJ/molHf NaNO3  aq   = -365.6 kJ/molNow, we can plug these values into the equation:H = [ -127.0 kJ/mol  +  -365.6 kJ/mol ] - [ -124.4 kJ/mol  +  -407.3 kJ/mol ]H =  -492.6 kJ/mol  -  -531.7 kJ/mol H = 39.1 kJ/molThe standard enthalpy change for the precipitation reaction between aqueous silver nitrate and aqueous sodium chloride to form solid silver chloride and aqueous sodium nitrate is 39.1 kJ/mol.