**Reaction and Calorimetry Problem**1. When 0.243 g of Mg metal is combined with enough HCl to make 100 mL of solution in a constant-pressure calorimeter, the following reaction occurs:\[\text{Mg} (s) + 2 \, \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2 (g)\]If the temperature of the solution increases from 23.0 °C to 34.1 °C as a result of this reaction, calculate the change in enthalpy (\( \Delta H \)) in kJ/mol of Mg. Assume that the solution has a specific heat of 4.18 J/g°C.

Given that , Mass of Mg metal =0.243g Intial temperature T1= 23.0°C Final temperature T2= 34.1°C…

1. When 0.243 g of Mg metal is combined with enough HCl to make 100 mL of solution in a constant-pressure calorimeter, the following reaction occurs: Mg(s) + 2 HCI(aq) → MgCl, (aq) + H2 (8) If the temperature of the solution increases from 23.0 °C to 34.1 °C as a result of this reaction, calculate AH in kJ/mol of Mg. Assume that the solution has a specific heat of 4.18 J/g-°C.

1. When 0.243 g of Mg metal is combined with enough HCl to make 100 mL of solution in a constant-pressure calorimeter, the following reaction occurs: Mg(s) + 2 HCI(aq) → MgCl, (aq) + H2 (8) If the temperature of the solution increases from 23.0 °C to 34.1 °C as a result of this reaction, calculate AH in kJ/mol of Mg. Assume that the solution has a specific heat of 4.18 J/g-°C.

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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