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7. 2.500 grams of metal X (molar mass = 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g °C. Assume a solution density of 1.00 g/mL and a perfect system.

7. 2.500 grams of metal X (molar mass = 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g °C. Assume a solution density of 1.00 g/mL and a perfect system.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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7. 2.500 grams of metal X (molar mass = 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g °C. Assume a solution density of 1.00 g/mL and a perfect system.
Transcribed Image Text:7. 2.500 grams of metal X (molar mass = 65.39 g/mole) was reacted with 100.0 mL of a 1.500 M HCI solution in a coffee cup calorimeter. The temperature went from 12.50 °C to 40.50 °C. Determine the reaction enthalpy per mole of metal X. The specific heat of the solution is 4.184 J/g °C. Assume a solution density of 1.00 g/mL and a perfect system.
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