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In an experiment, you are using Hess's Law and calorimetry to determine the molar enthalpy for the neutralization of solid potassium hydroxide: KOH(s) + HBr(aq) → H,O(1) + KBr(aq) In order to use Hess's Law you must calculate molar enthalpy changes for two other known reactions: (1) HBг(ag) + Kонад) —Н20() + KBrfaq) (2) КОНIS) - Кон аgд) a. In reaction (1), the following data was recorded: Observation Experimental Observations Quantity, of reactant 1 100-ml of 1.00 mol/L KOH(aq) Quantity of reactant 2 100-ml of 1.00 mol/L HBr(aq) Initial temperature 10 °C Final temperature 12.5°C Combine the volumes of quantity 1 and 2 to obtain the mass of the environment, assume the specific heat capacity of water. Calculate the molar enthalpy for the neutralization of KOH(aq). (1:3) b. In reaction (2), the following data was recorded: Observation Experimental Observations Quantity of KOH(s) 5.61 g KOH(s) 3.43J Enthalpy Change determined from calorimetry For reaction (2) determine the molar enthalpy for KOH(s) → KOH(aq). (1:3) c. Using Hess's Law determine the molar enthalpy for: KOH(s) + HBr(aq) H,O(1) + KBr(aq) (A:3) d. What molar enthalpies are exothermic and endothermic? Give numerical reasons for your answer. (A:2) e. If the volume of the reactants in reactant (1) were doubled, what would happen to the molar enthalpy for the target equation? (A:1). Give specific reasons for your answer. (C:2) f. What are some flaws with determining molar enthalpy for this reaction from calorimetry? (C:2)

In an experiment, you are using Hess's Law and calorimetry to determine the molar enthalpy for the neutralization of solid potassium hydroxide: KOH(s) + HBr(aq) → H,O(1) + KBr(aq) In order to use Hess's Law you must calculate molar enthalpy changes for two other known reactions: (1) HBг(ag) + Kонад) —Н20() + KBrfaq) (2) КОНIS) - Кон аgд) a. In reaction (1), the following data was recorded: Observation Experimental Observations Quantity, of reactant 1 100-ml of 1.00 mol/L KOH(aq) Quantity of reactant 2 100-ml of 1.00 mol/L HBr(aq) Initial temperature 10 °C Final temperature 12.5°C Combine the volumes of quantity 1 and 2 to obtain the mass of the environment, assume the specific heat capacity of water. Calculate the molar enthalpy for the neutralization of KOH(aq). (1:3) b. In reaction (2), the following data was recorded: Observation Experimental Observations Quantity of KOH(s) 5.61 g KOH(s) 3.43J Enthalpy Change determined from calorimetry For reaction (2) determine the molar enthalpy for KOH(s) → KOH(aq). (1:3) c. Using Hess's Law determine the molar enthalpy for: KOH(s) + HBr(aq) H,O(1) + KBr(aq) (A:3) d. What molar enthalpies are exothermic and endothermic? Give numerical reasons for your answer. (A:2) e. If the volume of the reactants in reactant (1) were doubled, what would happen to the molar enthalpy for the target equation? (A:1). Give specific reasons for your answer. (C:2) f. What are some flaws with determining molar enthalpy for this reaction from calorimetry? (C:2)

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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In an experiment, you are using Hess's Law and calorimetry to determine the molar enthalpy for the neutralization of solid potassium hydroxide: KOH(s) + HBr(aq) → H,O(1) + KBr(aq) In order to use Hess's Law you must calculate molar enthalpy changes for two other known reactions: (1) HBг(ag) + Kонад) —Н20() + KBrfaq) (2) КОНIS) - Кон аgд) a. In reaction (1), the following data was recorded: Observation Experimental Observations Quantity, of reactant 1 100-ml of 1.00 mol/L KOH(aq) Quantity of reactant 2 100-ml of 1.00 mol/L HBr(aq) Initial temperature 10 °C Final temperature 12.5°C Combine the volumes of quantity 1 and 2 to obtain the mass of the environment, assume the specific heat capacity of water. Calculate the molar enthalpy for the neutralization of KOH(aq). (1:3)
Transcribed Image Text:In an experiment, you are using Hess's Law and calorimetry to determine the molar enthalpy for the neutralization of solid potassium hydroxide: KOH(s) + HBr(aq) → H,O(1) + KBr(aq) In order to use Hess's Law you must calculate molar enthalpy changes for two other known reactions: (1) HBг(ag) + Kонад) —Н20() + KBrfaq) (2) КОНIS) - Кон аgд) a. In reaction (1), the following data was recorded: Observation Experimental Observations Quantity, of reactant 1 100-ml of 1.00 mol/L KOH(aq) Quantity of reactant 2 100-ml of 1.00 mol/L HBr(aq) Initial temperature 10 °C Final temperature 12.5°C Combine the volumes of quantity 1 and 2 to obtain the mass of the environment, assume the specific heat capacity of water. Calculate the molar enthalpy for the neutralization of KOH(aq). (1:3)
b. In reaction (2), the following data was recorded: Observation Experimental Observations Quantity of KOH(s) 5.61 g KOH(s) 3.43J Enthalpy Change determined from calorimetry For reaction (2) determine the molar enthalpy for KOH(s) → KOH(aq). (1:3) c. Using Hess's Law determine the molar enthalpy for: KOH(s) + HBr(aq) H,O(1) + KBr(aq) (A:3) d. What molar enthalpies are exothermic and endothermic? Give numerical reasons for your answer. (A:2) e. If the volume of the reactants in reactant (1) were doubled, what would happen to the molar enthalpy for the target equation? (A:1). Give specific reasons for your answer. (C:2) f. What are some flaws with determining molar enthalpy for this reaction from calorimetry? (C:2)
Transcribed Image Text:b. In reaction (2), the following data was recorded: Observation Experimental Observations Quantity of KOH(s) 5.61 g KOH(s) 3.43J Enthalpy Change determined from calorimetry For reaction (2) determine the molar enthalpy for KOH(s) → KOH(aq). (1:3) c. Using Hess's Law determine the molar enthalpy for: KOH(s) + HBr(aq) H,O(1) + KBr(aq) (A:3) d. What molar enthalpies are exothermic and endothermic? Give numerical reasons for your answer. (A:2) e. If the volume of the reactants in reactant (1) were doubled, what would happen to the molar enthalpy for the target equation? (A:1). Give specific reasons for your answer. (C:2) f. What are some flaws with determining molar enthalpy for this reaction from calorimetry? (C:2)
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