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3. If the value of the heat capacity (C) calculated in Part A of the experiment were too high, what effect would this have on your value for AHb, the enthalpy change for the reaction between magnesium metal and hydrochloric acid? Be specific. Would your answer be too high, or too low, and why?

3. If the value of the heat capacity (C) calculated in Part A of the experiment were too high, what effect would this have on your value for AHb, the enthalpy change for the reaction between magnesium metal and hydrochloric acid? Be specific. Would your answer be too high, or too low, and why?

Chemistry
Chemistry
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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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 If the value of the heat capacity (C) calculated in Part A of the experiment were too high, what effect would this have on your value for ΔHb, the enthalpy change for the reaction between magnesium metal and hydrochloric acid? Be specific. Would your answer be too high, or too low, and why? This are the question for reference, please consider it
1.Determine AH° for 2 Al (s) + 3/2 02 (g) → A|203 (s) Given AH° = -286 kJ/mol H2 (g) + ½ 02 (g) → H2O (I) 2 Al (s) + 6 H+ (ag) → 2 A13+ (ag) + 3 H2 (g) AH° = -1050 kJ/mol Al203 (s) + 6 H+ (ag) → 2 Al3+ (ag) + 3 H2O (g) AH° = -238 kJ/mol 2. Assume a coffee-cup calorimeter had a heat capacity (C) of 420 J/°C. If 1.00 g of Al2O3 completely reacted with HCI (H+ ) in the calorimeter, calculate the temperature change, AT. Hint: one of the reactions and AH values from question #1 may be helpful. Watch your units! MW (AI203) = 101.96 g/mol 3. If the value of the heat capacity (C) calculated in Part A of the experiment were too high, what effect would this have on your value for AHb, the enthalpy change for the reaction between magnesium metal and hydrochloric acid? Be specific. Would your answer be too high, or too low, and why? 4. Suppose that you used a metal container, rather than a Styrofoam cup, as the calorimeter. How might this affect the temperature-time curve? If the mass of the container and solvent is the same in both cases, will the heat capacity values be the same for both calorimeters? Explain your answers. 5. Sketch the temperature vs. time graph that you would expect for an endothermic reaction carried out in a calorimeter similar to the one used in the experiment (assume the reaction is not instantaneous and that the calorimeter is not perfectly insulated).
Transcribed Image Text:1.Determine AH° for 2 Al (s) + 3/2 02 (g) → A|203 (s) Given AH° = -286 kJ/mol H2 (g) + ½ 02 (g) → H2O (I) 2 Al (s) + 6 H+ (ag) → 2 A13+ (ag) + 3 H2 (g) AH° = -1050 kJ/mol Al203 (s) + 6 H+ (ag) → 2 Al3+ (ag) + 3 H2O (g) AH° = -238 kJ/mol 2. Assume a coffee-cup calorimeter had a heat capacity (C) of 420 J/°C. If 1.00 g of Al2O3 completely reacted with HCI (H+ ) in the calorimeter, calculate the temperature change, AT. Hint: one of the reactions and AH values from question #1 may be helpful. Watch your units! MW (AI203) = 101.96 g/mol 3. If the value of the heat capacity (C) calculated in Part A of the experiment were too high, what effect would this have on your value for AHb, the enthalpy change for the reaction between magnesium metal and hydrochloric acid? Be specific. Would your answer be too high, or too low, and why? 4. Suppose that you used a metal container, rather than a Styrofoam cup, as the calorimeter. How might this affect the temperature-time curve? If the mass of the container and solvent is the same in both cases, will the heat capacity values be the same for both calorimeters? Explain your answers. 5. Sketch the temperature vs. time graph that you would expect for an endothermic reaction carried out in a calorimeter similar to the one used in the experiment (assume the reaction is not instantaneous and that the calorimeter is not perfectly insulated).
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