**Calorimetry Experiment: Determining Specific Heat Capacity of Quartz**A 54.3 g sample of quartz is placed into a calorimeter, as illustrated in the adjacent sketch. The calorimeter contains 250.0 g of water. Initially, the quartz sample is at a temperature of 87.5 °C, while the water starts at 18.0 °C. When equilibrium is reached, the water's final temperature is 20.6 °C. The pressure remains constant at 1 atm throughout the experiment.**Objective:**Calculate the specific heat capacity of quartz based on this experimental setup. Ensure the answer is rounded to two significant digits.**Diagram Explanation:**The right side of the image shows a labeled diagram of a calorimeter. It includes:- A thermometer to measure the temperature.- An insulated container to minimize heat loss.- Water in which the quartz sample is submerged.Be sure to express the specific heat capacity in J/g·°C. Use the formula and insert values accordingly to compute the result.

Given: Mass of sample of quartz =54.6 g Mass of water = 250.0 g Initial temperature of quartz sample…

A 54.3 g sample of quartz is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The quartz sample starts off at 87.5 °C and the temperature of the water starts off at 18.0 °C. When the temperature of the water stops changing it's 20.6 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to 2 significant digits.

A 54.3 g sample of quartz is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The quartz sample starts off at 87.5 °C and the temperature of the water starts off at 18.0 °C. When the temperature of the water stops changing it's 20.6 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of quartz according to this experiment. Be sure your answer is rounded to 2 significant digits.

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.

Question

**Calorimetry Experiment: Determining Specific Heat Capacity of Quartz**

A 54.3 g sample of quartz is placed into a calorimeter, as illustrated in the adjacent sketch. The calorimeter contains 250.0 g of water. Initially, the quartz sample is at a temperature of 87.5 °C, while the water starts at 18.0 °C. When equilibrium is reached, the water's final temperature is 20.6 °C. The pressure remains constant at 1 atm throughout the experiment.

**Objective:**
Calculate the specific heat capacity of quartz based on this experimental setup. Ensure the answer is rounded to two significant digits.

**Diagram Explanation:**
The right side of the image shows a labeled diagram of a calorimeter. It includes:
- A thermometer to measure the temperature.
- An insulated container to minimize heat loss.
- Water in which the quartz sample is submerged.

Be sure to express the specific heat capacity in J/g·°C. Use the formula and insert values accordingly to compute the result.

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