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How does the heat or enthalpy of the reaction (ΔHrxn) change when the concentration of a Strong acid (HCl) is increasing and the concentration of strong base (NaOH) is kept constant in a solution mixture?

How does the heat or enthalpy of the reaction (ΔHrxn) change when the concentration of a Strong acid (HCl) is increasing and the concentration of strong base (NaOH) is kept constant in a solution mixture?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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How does the heat or enthalpy of the reaction (ΔHrxn) change when the concentration of a Strong acid (HCl) is increasing and the concentration of strong base (NaOH) is kept constant in a solution mixture?

plz answer showing the steps to solve quantatiavely using hess's law. ive also attached images of my lab data for reference

a) (msolution) = total mass (msolution) = 106.764g – 3.509g = 103.255g b) AT = Tt - Ti AT = 24.30°C – 17.75°C = 6.550°C c) q = m*Cs* AT q = 0.103255kg * 4.184kJ/K*6.550°C = 3.56966kJ d) n(HCI) = (0.923mol/L)(50mL)(1L/1000mL) = 0.046mol n(NaOH) = (0.955mol/L)(50mL)(1L/1000OmL) = 0.048mol According to the balanced equation: HCI(aq)+NaOH(aq)→NaCI(aq)+H 20(1), the stoichiometric ratio between the moles of HCl and the product moles of H20 produced is of a 1:1 ratio, thus 0.046mol of HCI will react with 0.048mol of NaOH to produce 0.046mol of H2O mass of cups
Transcribed Image Text:a) (msolution) = total mass (msolution) = 106.764g – 3.509g = 103.255g b) AT = Tt - Ti AT = 24.30°C – 17.75°C = 6.550°C c) q = m*Cs* AT q = 0.103255kg * 4.184kJ/K*6.550°C = 3.56966kJ d) n(HCI) = (0.923mol/L)(50mL)(1L/1000mL) = 0.046mol n(NaOH) = (0.955mol/L)(50mL)(1L/1000OmL) = 0.048mol According to the balanced equation: HCI(aq)+NaOH(aq)→NaCI(aq)+H 20(1), the stoichiometric ratio between the moles of HCl and the product moles of H20 produced is of a 1:1 ratio, thus 0.046mol of HCI will react with 0.048mol of NaOH to produce 0.046mol of H2O mass of cups
Table 1: Trial Data Mass of cups (g) Volume of HCI (mL) Volume of NaOH (mL) 3.509 50 50 NaOH concentration (M) 0.955 Initial temperature of compounds (°C) 17.75 Trial #1 Trial #2 Trial #3 HCl concentration (M) 0.923 0.692 0.462 Final temperature of compounds (°C) Mass of solution (kg) 24.3 22.8 21.2 0.103255 0.10199 0.102134 AT (°C) 6.55 5.05 3.35 Energy/q (kJ) Change in enthalphy/AHrxn (kJ/mol) 3.57 2.15 1.43 -55.83 -55.83 -55.83
Transcribed Image Text:Table 1: Trial Data Mass of cups (g) Volume of HCI (mL) Volume of NaOH (mL) 3.509 50 50 NaOH concentration (M) 0.955 Initial temperature of compounds (°C) 17.75 Trial #1 Trial #2 Trial #3 HCl concentration (M) 0.923 0.692 0.462 Final temperature of compounds (°C) Mass of solution (kg) 24.3 22.8 21.2 0.103255 0.10199 0.102134 AT (°C) 6.55 5.05 3.35 Energy/q (kJ) Change in enthalphy/AHrxn (kJ/mol) 3.57 2.15 1.43 -55.83 -55.83 -55.83
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