How much heat was absorbed by the solution?What is the enthalpy of the reaction? A generic solid, X, has a molar mass of 83.3 g/mol. In a constant-pressure calorimeter, 17.2 g of X is dissolved in 219 g of water at 23.00 °C.\[ \text{X(s)} \rightarrow \text{X(aq)} \]The temperature of the resulting solution rises to 27.00 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings.**How much heat was absorbed by the solution?**\[ q = \]- The given answer is \( 3.953 \times 10^3 \) kJ (Incorrect).**What is the enthalpy of the reaction?**\[ \Delta H_{\text{rxn}} = \]- This answer is required in kJ/mol (Incorrect).*Explanation:*- **Calculation of q (heat absorbed):** The question asks for the heat absorbed by the solution, which is typically calculated using the formula: \[ q = m \cdot c \cdot \Delta T \] where \( m \) is the mass, \( c \) is the specific heat, and \( \Delta T \) is the change in temperature. - **Enthalpy of reaction calculation:** The enthalpy change of the reaction, \( \Delta H_{\text{rxn}} \), involves using the heat absorbed and considering the moles of substance involved in the reaction for a molar perspective.

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A generic solid, X, has a molar mass of 83.3 g/mol. In a constant-pressure calorimeter, 17.2 g of X is dissolved in 219 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 27.00 °C. Assume the solution has the same specific heat as water, 4.184 J/(g-°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? 3.953 x103 q = kJ Incorrect What is the enthalpy of the reaction? AHrxn kJ/mol Incorrect

A generic solid, X, has a molar mass of 83.3 g/mol. In a constant-pressure calorimeter, 17.2 g of X is dissolved in 219 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 27.00 °C. Assume the solution has the same specific heat as water, 4.184 J/(g-°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? 3.953 x103 q = kJ Incorrect What is the enthalpy of the reaction? AHrxn kJ/mol Incorrect

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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