In a coffee-cup calorimeter, 110.0 mL of 1.2 MNaOH and 110.0 mL of 1.2 MHCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a densityof 1.03g/cm³ and a specific heat capacity of 4.18 J/°C∙g, calculate the enthalpy change for the neutralization ofHCl byNaOH. Assume that no heat is lost to the surroundings or to the calorimeter.AH =kJ/mol A 149.5-g sample of a metal at 75.5°C is added to 149.5 g H₂O at 15.6°C. The temperature of the water rises to 18.1°C. Calculate the specific heat capacityof the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C.g.Specific heat capacity = 0.056J/°C.g

Mass of Water, m = 149.5 gspecific heat of water, s = 4.184 J/goCinitial temperature, T1 = 15.6…

A 149.5-g sample of a metal at 75.5°C is added to 149.5 g H₂O at 15.6°C. The temperature of the water rises to 18.1°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C.g. Specific heat capacity = 0.056 J/°C-g

A 149.5-g sample of a metal at 75.5°C is added to 149.5 g H₂O at 15.6°C. The temperature of the water rises to 18.1°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C.g. Specific heat capacity = 0.056 J/°C-g

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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