CHEM Act B5 HEAT-SI Lab Report Heat Relationships in Physical and Chemical Processes Answered 2024.

CHEM Act B5 HEAT-SI Lab Report Heat Relationships in Physical and Chemical Processes Answered 2024. Act B5 HEAT-SI Lab Report Heat Relationships in Physical and Chemical Processes Parts I - III Act B5 Online URL: The computer will simulate a calorimetry experiment involving dissolving various ionic salts in water. The following compounds should be available for testing: ammonium nitrate, sodium nitrate, calcium nitrate, magnesium nitrate, sodium chloride, calcium chloride, ammonium chloride, magnesium chloride. Part I Measure Heat of a Physical Process Test all eight of the compounds using the same mass value for each. Some of your compounds may cause an increase in temperature of the solution, other compounds could cause a decrease in the temperature of the solution. Write a specific question that you can answer as a result of performing your calorimetry experiment. Part I A. Design and carry out an experiment to determine the change in enthalpy, DH (kJ), for the dissolving process for these ionic solids. 1. Write the chemical formulas for these ionic solids. Ionic Solid Chemical Formula Ammonium nitrate NH4NO3 Lithium chloride LiCl Calcium chloride CaCl2 Potassium chloride KCl Sodium chloride NaCl 2. In your experiment, identify the independent and dependent variables. The dependent variable is change in temperature, and the independent variable is the ionic salts. 3. What is the magnitude and unit of the control variable in your experiment? The control variable in my experiment is the mass of the compound and volume of water. Each salt obtained a mass of 0.5g and a volume of water of 20mL. 4. Write equations that describe the dissolving process for each salt. Classify each process as endothermic, exothermic, or neither after collecting the data. Ionic Solid Chemical Equation Type Energy Change Lithium chloride LiCl(s)+H2O(l)=Li^+(aq)+Cl^-(aq) Exothermic Calcium chloride CaCl2(s)+H2O(l)=Ca2^+(aq)+2Cl^-(aq) Exothermic Potassium chloride KCl(s)+H2O(l)=K^+9aq)+Cl^-(aq) Exothermic Sodium chloride NaCl(s)+H2O(l)=K^+(aq)+Cl^-(aq) Exothermic 5. List the assumptions and or information that you need to make in order to do the calculations. The information needed to perform the calculations are the number of moles, pressure, and volume. Furthermore, the assumptions are that no heat is gained nor lost. 6. In your experiment, identify the system. The system is any activity in the calorimeter. 7. In your experiment identify the surroundings. The surroundings would include any activity outside the calorimeter. 8. In your experiment, what gains heat energy? In the experiment, the endothermic reactions are what gains heat energy. 9. In your experiment what loses heat energy? In the experiment, the exothermic reactions are what loses energy. 10. Report the heat of reaction (qRxn) for each ionic solid. Show your calculation or each salt. Report the final value in Joules. Ionic Solid Calculation qRxn (J) Ammonium nitrate (4.184J/g*C)(20.5g)(-1.91C) -163.82J Lithium chloride (4.184J/g*C)(20.5g)(5.1C) 434.44J Calcium chloride (4.184J/g*C)(20.5g)(4.34C) 372.25J Potassium chloride (4.184J/g*C)(20.5g)(-1.35C) -122.97J Sodium chloride (4.184J/g*C)(20.5g)(-0.4C) -34.31J.