A 100 ml sample of .200 M aqueous hydrochloric acid is addedto 100 ml of .200 M

Question

A 100 ml sample of .200 M aqueous hydrochloric acid is addedto 100 ml of .200 M aqueous ammonia in a calorimeter whose heatcapacity (excluding any water) is 480 J/K. The following reactionoccurs when the two solutions are mixed. HCl(aq) + NH3 (aq) yields NH4Cl(aq) The temperature increase is 2.34 degrees celcius. CalculateH per mole of HCl and NH3 reacted. A 100 ml sample of .200 M aqueous hydrochloric acid is addedto 100 ml of .200 M aqueous ammonia in a calorimeter whose heatcapacity (excluding any water) is 480 J/K. The following reactionoccurs when the two solutions are mixed. HCl(aq) + NH3 (aq) yields NH4Cl(aq) The temperature increase is 2.34 degrees celcius. CalculateH per mole of HCl and NH3 reacted.

Explanation / Answer

       The given reaction is    Mixing solution of HCl and NH3 resultsin acid Base reaction .    HCl(aq) + NH3 (aq) --------->NH4Cl (aq) The total heat produced can be calculated usingqrxn= -Cs-m*t Here the number of moles of HCl consumed in thereaction bust be calculated from the Volume and molarity of thissubstance .And ths amount then used to determine the Heat producedper mole of HCl. Because the total Volume of the solution is 200.0 mLits mass is    = (200mL)(1.5g /mL)=300g                                        (Density of NH4Cl=1.5g /mL) The temperature Change T=2.340C    From the above reaction qrxn= (480 J/gK.)(300g)(2.34 k)                                                 =336960 J                                                 =336.960 kJ Because the process Occur at constant pressureH=336.960kJ        To express the enthalpychange on a molar mass we use the fact that the number of moles ofHCl is given by the number of moles HCl is given by the product ofthe respective solution volume 100 mL=0.100LAnd the concentration0.200M=0.200mol/L                  = (0.100L)(0.200mol/L)=0.02 mol                         Enthalpy =336.960kJ /0.02 mol=16848 kJ/mol Because the process Occur at constant pressureH=336.960kJ        To express the enthalpychange on a molar mass we use the fact that the number of moles ofHCl is given by the number of moles HCl is given by the product ofthe respective solution volume 100 mL=0.100LAnd the concentration0.200M=0.200mol/L                  = (0.100L)(0.200mol/L)=0.02 mol                         Enthalpy =336.960kJ /0.02 mol=16848 kJ/mol   

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