Question

Procedure 1 Hydration of Ammonium Chloride View the video by clicking HERE. 1. Measure 25 mL of deionized water using a graduated cylinder and place it into the calorimeter. Record the temperature of the water. 2. Weigh 4.83 g of ammonium chloride, NH,Cl, on a top loading balance. Add this, w stirring, to the water in the calorimeter. Record the final temperature of the mixture. Initial Temperature 19.8 Final Temperature 6.8 Be sure to include the correct sign (+ or -) for each value you enter! Change in Temperature -13 Vol of water used = mass of water 25 4H20 - Click to enlter value Arxn - Click to enter value moles of NH CI - Click to enter value AH --Click to enter value J/mol = Click to enter value kJ/mol The actual enthalpy of hydration for NH CI is AH - +14.6 kJ/mol. Calculate the percent error. Percent Error - x 100% % error - Click to enter value /2.5 pts MacBook Air

Answer 1

To calcualte the dissolution of the reaction we supposed to use the heat equaiton given below

Q = mc∆T

Q = heat in Joules   

m = mass the solution (g) = 29.83 g

c = specific heat = 4.184 J/g∙°C

∆T = difference in temperature (°C ) = 13 °C

Heat gained by the reaction is equal to heat lost by the solution

we can calculate heat the lost by the solution using the above formula

QH2O = 29.83 gm x 4.184 J/g∙°C x 13 °C =  1,622.51 Joules

The heat released by the solution (Q H2O ) =1622.51 J

Q rxn =  1622.51 J   = 1622 J

Moles of NH4Cl   = 4.83 g / 53.49 g/mol = 0.0903 Moles

ΔH of NH4Cl  =  1622 J / 0.0903 Mole = 17963 J /Mole =  17.96 kJ /Mole