### Thermochemistry Problems#### Question 11:**Problem Statement:**A piece of metal weighing 3.20 grams is heated to 100.0°C. It is dropped into 50.0 grams of water in a calorimeter at 22.5°C. When no further change is observed, the temperature of the water and the metal rod is 26.5°C. Ignoring any heat lost or gained by the calorimeter, what is the metal and its specific heat?**Options:**a. Cu, 0.39 J g⁻¹ K⁻¹ b. Hg, 0.14 J g⁻¹ K⁻¹ c. Pb, 0.13 J g⁻¹ K⁻¹ d. Na, 1.2 J g⁻¹ K⁻¹ e. Li, 3.6 J g⁻¹ K⁻¹ **Letter answer to question #11: _______**#### Question 12:**Problem Statement:**Calculate the amount of heat needed to change 45.0 grams of ice at -25.0°C to steam at 250.0°C. (For water, ΔH_fus = 333 J/g; ΔH_vap = 2260 J/g; Specific Heat (ice) = 2.10 J g⁻¹ K⁻¹; Specific Heat (steam) = 2.00 J g⁻¹ K⁻¹)**Options:**a. 14.7 kJ b. 33.7 kJ c. 116 kJ d. 151 kJ e. 175 kJ **Letter answer to question #12: _______**#### Explanation of Concepts:**Calorimetry:**Calorimetry is a branch of thermochemistry that deals with measuring the heat evolved or absorbed during a chemical reaction, physical change, or heat capacity. The basic process involves measuring the temperature change of a substance when subjected to heating or cooling. **Phase Change Calculations:**1. To calculate the heat needed to change ice at a specific temperature to steam, one must account for the energy required for each of the following steps: - Heating the ice to its melting point (0°C) - Melting the ice to water - Heating the water to its boiling point (100°C)

11) Mass of the piece of metal = 3.20 grams Temperature= 100o CMass of water in calorimeter = 50…

11. A piece of metal weighing 3.20 grams is heated to 100. °C. It is dropped into 50.0 grams of water in a calorimeter at 22.5 °C. When no further change is observed, the temperature of the water and the metal rod is 26.5 °C. Ignoring any heat lost or gained by the calorimeter, what is the metal and its specific heat? a. Cu, 0.39 J g-1 K-1 b. Hg, 0.14 J g-¹ K-¹ c. Pb, 0.13 Jg¹ K-¹ d. Na, 1.2 Jg-¹ K-¹ e. Li, 3.6 Jg-¹ K-1 Letter answer to question #11:

11. A piece of metal weighing 3.20 grams is heated to 100. °C. It is dropped into 50.0 grams of water in a calorimeter at 22.5 °C. When no further change is observed, the temperature of the water and the metal rod is 26.5 °C. Ignoring any heat lost or gained by the calorimeter, what is the metal and its specific heat? a. Cu, 0.39 J g-1 K-1 b. Hg, 0.14 J g-¹ K-¹ c. Pb, 0.13 Jg¹ K-¹ d. Na, 1.2 Jg-¹ K-¹ e. Li, 3.6 Jg-¹ K-1 Letter answer to question #11:

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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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

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