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4. 56.0 ml of 1.5 M HCl is mixed with 68.5 mL of 1.33 M NAOH in a calorimeter cup (C= 55.35 J/ C) If the initial temperatures of both solutions before mixing is 21.78°C determine the final temperature of the combined solutions after the reaction takes place. Step 1: Determine the moles of HCl and NaOH present and clearly identify the limiting reactant. Show all calculations. Step 2: Use the limiting reactant and AH,n=-57.62 kJ/mole to determine the heat released by the reaction. Show all calculations. Step 3: Use the heat you determined in Step 2 to calculate the temperature change using m.olution X Celution X AT the equation: Ca x AT. Assume the solution has the same density and specific heat as pure water. Show all calculations. Step 4: Assuming the initial temperature of the two solutions is 21.78 C, determine the final temperature of the total solution. Show all calculations.

4. 56.0 ml of 1.5 M HCl is mixed with 68.5 mL of 1.33 M NAOH in a calorimeter cup (C= 55.35 J/ C) If the initial temperatures of both solutions before mixing is 21.78°C determine the final temperature of the combined solutions after the reaction takes place. Step 1: Determine the moles of HCl and NaOH present and clearly identify the limiting reactant. Show all calculations. Step 2: Use the limiting reactant and AH,n=-57.62 kJ/mole to determine the heat released by the reaction. Show all calculations. Step 3: Use the heat you determined in Step 2 to calculate the temperature change using m.olution X Celution X AT the equation: Ca x AT. Assume the solution has the same density and specific heat as pure water. Show all calculations. Step 4: Assuming the initial temperature of the two solutions is 21.78 C, determine the final temperature of the total solution. Show all calculations.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.109QP: A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter...
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4. 56.0 ml of 1.5 M HCl is mixed with 68.5 mL of 1.33 M NAOH in a calorimeter cup (C= 55.35 1/°C) If the initial temperatures of both solutions before mixing is 21.78°C determine the final temperature of the combined solutions after the reaction takes place. Step 1: Determine the moles of HCl and NaOH present and clearly identify the limiting reactant. Show all calculations. Step 2: Use the limiting reactant and AH= -57.62 kJ/mole to determine the heat released by the reaction. Show all calculations. Step 3: Use the heat you determined in Step 2 to calculate the temperature change using the equation: gon = m.olution X Clution X AT Ceat x AT. Assume the solution has the same density and specific heat as pure water. Show all calculations. Step 4: Assuming the initial temperature of the two solutions is 21.78 °C, determine the final temperature of the total solution. Show all calculations.
Transcribed Image Text:4. 56.0 ml of 1.5 M HCl is mixed with 68.5 mL of 1.33 M NAOH in a calorimeter cup (C= 55.35 1/°C) If the initial temperatures of both solutions before mixing is 21.78°C determine the final temperature of the combined solutions after the reaction takes place. Step 1: Determine the moles of HCl and NaOH present and clearly identify the limiting reactant. Show all calculations. Step 2: Use the limiting reactant and AH= -57.62 kJ/mole to determine the heat released by the reaction. Show all calculations. Step 3: Use the heat you determined in Step 2 to calculate the temperature change using the equation: gon = m.olution X Clution X AT Ceat x AT. Assume the solution has the same density and specific heat as pure water. Show all calculations. Step 4: Assuming the initial temperature of the two solutions is 21.78 °C, determine the final temperature of the total solution. Show all calculations.
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