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Chapter 9: Problem 58

Could an endothermic reaction be used to determine the heat capacity of a calorimeter?

Short Answer

Expert verified
If so, how? Answer: Yes, an endothermic reaction can be used to determine the heat capacity of a calorimeter. In this case, the temperature of the substance inside the calorimeter would decrease as the reaction absorbs heat from it. By measuring the temperature change and using the heat capacity of the substance, we can calculate the amount of heat absorbed by the reaction. Then, we can use this information to determine the heat capacity of the calorimeter.

Step by step solution

01

Understand endothermic reactions

An endothermic reaction is a chemical reaction that absorbs heat from the surroundings. In other words, the energy is transferred from the surroundings into the system, causing the temperature of the surroundings to drop.
02

Calorimetry

Calorimetry is an experimental technique used to measure the heat capacity of a system, which is usually a calorimeter. A calorimeter is an insulated container used to minimize heat transfer between the system and its surroundings. It typically contains a thermometer, a stirrer, and a known mass of a substance, often water. The calorimeter is used to measure the heat absorbed or released during a reaction taking place inside the calorimeter.
03

Determining heat capacity using an exothermic reaction

When an exothermic reaction (a reaction that releases heat) occurs within a calorimeter, the heat released by the reaction is absorbed by the calorimeter and the substance inside it (usually water). By measuring the change in temperature of the substance inside the calorimeter, we can determine the heat released by the reaction. We can then use this information to calculate the heat capacity of the calorimeter, which is the amount of heat required to raise the temperature of the calorimeter by one degree Celsius.
04

Can an endothermic reaction be used?

Yes, an endothermic reaction can also be used to determine the heat capacity of a calorimeter, but the process would be slightly different. Instead of measuring the heat released by the reaction, we would measure the heat absorbed by the reaction from the calorimeter and the substance inside it. In this case, the temperature of the substance inside the calorimeter would decrease as the reaction absorbs heat from it. By measuring the temperature change and using the heat capacity of the substance, we can calculate the amount of heat absorbed by the reaction. Then, we can use this information to determine the heat capacity of the calorimeter. In conclusion, both exothermic and endothermic reactions can be used to determine the heat capacity of a calorimeter. It is essential to understand the differences between exothermic and endothermic reactions and to carefully measure the temperature changes during the reaction to accurately calculate the heat capacity of the calorimeter.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Endothermic Reactions
Endothermic reactions play a fascinating role in the realm of chemistry by absorbing heat from their surroundings. This absorption is a form of energy transfer, where the system (the area where the reaction occurs) intakes energy, leading to a temperature drop in the nearby environment. Due to this distinctive characteristic, endothermic reactions are the inverse of exothermic reactions, which instead release heat. Some common examples of endothermic reactions include ice melting and photosynthesis, processes where energy absorption is essential for transformation.
  • Energy is taken in by the system.
  • The surrounding temperature decreases.
  • Endothermic processes often involve noticeable phase changes or energy requirements.
Understanding endothermic reactions is crucial when dealing with calorimetry because they require precise measurements of the heat absorbed to determine caloric changes. Mastering this knowledge aids in comprehending how energy and temperature interact during various chemical reactions.
Heat Capacity
Heat capacity is a fundamental concept in thermodynamics that describes how much heat an object or substance can hold. It indicates the amount of heat energy needed to raise the temperature of a substance by one degree Celsius. This property is critical in experiments involving calorimetry, as it helps scientists gauge how different materials and systems respond to heat changes. For example, the heat capacity of a calorimeter itself is vital to making accurate measurements.
  • Expressed as the change in temperature per unit of heat.
  • Crucial for calculating heat changes in reactions.
  • Varies between substances due to differing physical properties, such as mass and specific heat capacity.
By understanding the heat capacity, one can determine the specific heat for substances. This knowledge allows for the calculation of energy transfers, especially important when studying both endothermic and exothermic reactions for practical applications in laboratory settings.
Thermal Equilibrium
Thermal equilibrium happens when two objects or systems in contact with each other reach the same temperature, leading to no net heat flow between them. This state is essential in calorimetry because the calorimeter and its contents must equilibrate with any reactions taking place to ensure precise measurement of energy changes.
  • Essential for accurate calorimetric measurements.
  • No further energy exchange occurs at equilibrium.
  • Both the system and surroundings remain stable in temperature.
In calorimetry, reaching thermal equilibrium signifies the completion of energy transfer between the substance undergoing the reaction and its environment. This balance allows scientists to measure the heat associated with chemical reactions accurately, giving insight into the total thermal energy involved. Specifically, determining the heat capacity through calorimetry relies on achieving and identifying this equilibrium state.

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Most popular questions from this chapter

Breaking the small pouch of water inside a chemical cold pack containing ammonium nitrate activates the pack, which is used by sports trainers for injured athletes. What is the sign of \(\Delta H\) for the process taking place in the cold pack?

The destruction of the ozone layer by chlorofluorocarbons (CFCs) can be described by the following reactions: $$\begin{aligned}\mathrm{ClO}(g)+\mathrm{O}_{3}(g) & \rightarrow \mathrm{Cl}(g)+2 \mathrm{O}_{2}(g) & \Delta H_{\mathrm{rxn}}^{\circ} &=-29.90 \mathrm{kJ} \\\2 \mathrm{O}_{3}(g) \rightarrow 3 \mathrm{O}_{2}(g) & & \Delta H_{\mathrm{rxn}}^{\circ} &=+24.18 \mathrm{kJ}\end{aligned}$$ Use the preceding \(\Delta H_{\mathrm{rxn}}^{\circ}\) values to determine the value of the standard heat of reaction for this reaction: $$\mathrm{Cl}(g)+\mathrm{O}_{3}(g) \rightarrow \mathrm{ClO}(g)+\mathrm{O}_{2}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=?$$

The mineral spodumene \(\left(\operatorname{LiAlSi}_{2} \mathrm{O}_{6}\right)\) exists in two crystalline forms called \(\alpha\) and \(\beta .\) Use Hess's law and the following information to calculate \(\Delta H_{\mathrm{rxn}}^{\circ}\) for the conversion of \(\alpha\) -spodumene into \(\beta\) -spodumene: $$\begin{array}{r}\mathrm{Li}_{2} \mathrm{O}(s)+2 \mathrm{Al}(s)+4 \mathrm{SiO}_{2}(s)+\frac{3}{2} \mathrm{O}_{2}(g) \rightarrow 2 \alpha-\mathrm{LiAlSi}_{2} \mathrm{O}_{6}(s) \\ \Delta H_{\mathrm{rxn}}^{\circ}=-1870.6 \mathrm{kJ} \end{array}$$ $$\begin{array}{r}\mathrm{Li}_{2} \mathrm{O}(s)+2 \mathrm{Al}(s)+4 \mathrm{SiO}_{2}(s)+\frac{3}{2} \mathrm{O}_{2}(g) \rightarrow 2 \beta-\mathrm{LiAlSi}_{2} \mathrm{O}_{6}(s) \\\\\Delta H_{\mathrm{rxn}}^{\circ}=-1814.6 \mathrm{kJ} \end{array}$$

How is Hess's law consistent with the law of conservation of energy?

In a simple "kitchen chemistry" experiment, some vinegar is poured into an empty soda bottle. A deflated balloon containing baking soda is stretched over the mouth of the bottle. Holding up the balloon and shaking it allows the baking soda to fall into the vinegar, which starts the following reaction and inflates the balloon: $$\begin{aligned} \mathrm{NaHCO}_{3}(a q)+\mathrm{CH}_{3} \mathrm{COOH}(a q) \rightarrow & \\ & \mathrm{CH}_{3} \mathrm{COONa}(a q)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(\ell) \end{aligned}$$ If the contents of the bottle are the system, is work being done on the surroundings or on the system?
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