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What is the change in enthalpy (in kJ/mol) for the reaction below, if 2.666 g of Zn reacting with excess concentrated HCI caused the solution's temperature to increase from 21.1 °C to 35.0 °C? The volume of the solution is 120.0 mL. Use the specific heat and density of water, 4.184 J g-¹1 °C-1 and 1.00 g/mL, respectively. Your Answer:

What is the change in enthalpy (in kJ/mol) for the reaction below, if 2.666 g of Zn reacting with excess concentrated HCI caused the solution's temperature to increase from 21.1 °C to 35.0 °C? The volume of the solution is 120.0 mL. Use the specific heat and density of water, 4.184 J g-¹1 °C-1 and 1.00 g/mL, respectively. Your Answer:

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
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What is the change in enthalpy (in kJ/mol) for the reaction below, if 2.666 g of Zn reacting with excess concentrated HCI caused the solution's temperature to increase from 21.1 °C to 35.0 °C? The volume of the solution is 120.0 mL. Use the specific heat and density of water, 4.184 J g-¹ °C-1 and 1.00 g/mL, respectively. Your Answer: Answer units
Transcribed Image Text:What is the change in enthalpy (in kJ/mol) for the reaction below, if 2.666 g of Zn reacting with excess concentrated HCI caused the solution's temperature to increase from 21.1 °C to 35.0 °C? The volume of the solution is 120.0 mL. Use the specific heat and density of water, 4.184 J g-¹ °C-1 and 1.00 g/mL, respectively. Your Answer: Answer units
Expert Solution
Step 1

Given data

Zn Mass= 2.666 g   

volume of solution= 120 ml 

T1= 21.1 c

T2= 35.0 c

Specific heat =4.184 J g^-1 C^-1 

Density = 1 g/mL

Find delta H

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