Question

2. Consider the reaction of 50.0 mL of 1.15 M HC2H302 with 50.0 mL of 1.30 M NH3. a. Give the net ionic reaction between these two reagents. H+(99) + NH3(aq) →NH4+(29) b. Calculate the moles of each reactant and indicate which reactant is the limiting reagent. Moles of HC2H2O2: 0.058 moles Moles of NH3: 0.065 moles c. Once the two reactant solutions are brought to the same initial temperature, they are mixed in a calorimeter, also at the same initial temperature. A student carefully monitored the temperature and determined that the temperature of the two solutions and the calorimeter increased together by 6.50 °C. Knowing the heat capacity of the calorimeter is 54.0 J/°C, determine the heat of this reaction in kJ/mol. Use: -9.rso = 9:01+ goal and Hungar/moles and the following assumptions: 1. The solutions both have a density of 1.00g/mL, so 50.0mL - 50.0g for each solution 2. The solutions both have the same specific heat as water, 4.184 J/g-°C.