When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: • The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL • The liquid's final volume is not changed by adding the solid • The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change.
When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from 21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process. AX (s) → A*(aq) + X¯ (aq) Assumptions for this calculation: • The specific heat of the solution is the same as that of pure water (4.18 J/gK) • The density of water = 1.000 g/mL • The liquid's final volume is not changed by adding the solid • The calorimeter loses only a negligible quantity of heat. The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from
21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process.
AX (s) → A*(aq) + X- (aq)
Assumptions for this calculation:
· The specific heat of the solution is the same as that of pure water (4.18 J/gK)
• The density of water = 1.000 g/mL
· The liquid's final volume is not changed by adding the solid
· The calorimeter loses only a negligible quantity of heat.
The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change.
Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question,
enter your response to four decimal places. Carmen may add or remove digits from your response, your
submission will still be graded correctly if this happens.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F02ac992c-59f5-4674-9c6f-05ab0e575bae%2Fadc38db7-6f7b-49df-82ef-b75a653a4f08%2F2rrbe7_processed.png&w=3840&q=75)
Transcribed Image Text:When 2.89 g of AX (s) dissolves in 125.3 g of water in a coffee-cup calorimeter the temperature rises from
21.4 °C to 33.6 °C. Calculate the enthalpy change (in kJ/mol) for the solution process.
AX (s) → A*(aq) + X- (aq)
Assumptions for this calculation:
· The specific heat of the solution is the same as that of pure water (4.18 J/gK)
• The density of water = 1.000 g/mL
· The liquid's final volume is not changed by adding the solid
· The calorimeter loses only a negligible quantity of heat.
The formula weight of AX = 59.1097 g/mol. Be sure you include the correct sign for the enthalpy change.
Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question,
enter your response to four decimal places. Carmen may add or remove digits from your response, your
submission will still be graded correctly if this happens.
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