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Plants and living beings are examples of (a) isolated system (b) adiabatic system (c) open system (d) closed system

Short Answer

Expert verified
Plants and living beings are examples of an open system.

Step by step solution

01

Understand System Types

We first need to understand the different types of systems: - An **isolated system** does not exchange matter or energy with its surroundings. - An **adiabatic system** does not exchange heat with its surroundings but can exchange work. - An **open system** can exchange both matter and energy with its surroundings. - A **closed system** can exchange energy but not matter with its surroundings.
02

Analyze the Characteristics of Plants and Living Beings

Plants and living beings require inputs from the environment (like air, water, and nutrients) and also release substances back into the environment (like oxygen and waste). They also exchange energy with their surroundings in the form of light and heat.
03

Identify the System Type for Plants and Living Beings

Considering the characteristics identified in Step 2, plants and living beings exchange both matter and energy with their surroundings. This aligns with the definition of an **open system**.
04

Conclusion

Since plants and living beings match the characteristics of an open system, the correct choice is option (c) open system.

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Key Concepts

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

Thermodynamics
Thermodynamics is the branch of physics dealing with the study of the relationship between heat, work, and energy. It describes how energy moves through different systems and provides insights into how physical processes occur. In thermodynamics, we investigate the laws governing these energy exchanges and how systems communicate energetically with their surroundings.
Key concepts in thermodynamics include:
  • First Law: Energy cannot be created or destroyed, only transformed from one form to another.
  • Second Law: Entropy, a measure of disorder, always tends to increase, meaning energy processes increase the disorder of the universe.
  • Third Law: As temperature approaches absolute zero, the entropy of a system approaches a constant value.
The understanding of how energy transfers in the form of heat and work are fundamental. This is particularly important when identifying different kinds of systems, such as our open systems like plants and animals, which partake in such energetic exchanges constantly.
System Types
Understanding system types is crucial in thermodynamics, as they determine how a system interacts with its environment. The different system types are:
  • Isolated System: Does not exchange energy or matter with the environment. It is entirely self-contained.
  • Adiabatic System: Does not exchange heat with the surroundings but can exchange work, typically seen in insulated processes.
  • Open System: Freely exchanges both energy and matter with its surroundings. Examples include living organisms like plants and animals.
  • Closed System: Exchanges energy but not matter with its environment. A sealed steam radiator is a classic example.
For living organisms such as plants and animals, the constant exchange of nutrients, gases, and energy with their surroundings makes them open systems. They both take in materials such as water and oxygen, and emit waste products, as well as transfer energy in the form of heat.
Exchange of Matter and Energy
The concept of exchange of matter and energy is pivotal when discussing open systems, as illustrated by living beings and plants. This exchange enables biological processes essential for life.
  • Exchange of Matter: This involves the absorption and emission of substances like oxygen, carbon dioxide, water, and nutrients. Plants, for example, absorb carbon dioxide and release oxygen during photosynthesis.
  • Exchange of Energy: Involves capturing and utilizing energy from the environment. Plants convert sunlight into energy via photosynthesis, while animals consume plants or other organisms to obtain energy.
These exchanges are crucial as they allow organisms to sustain themselves and maintain life processes. The energy is used for growth, repair, and reproduction, while matter exchange facilitates metabolism and biochemical reactions.

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Most popular questions from this chapter

Which of the following equations represent standard heat of formation of \(\mathrm{C}_{2} \mathrm{H}_{4} ?\) (a) \(2 \mathrm{C}\) (diamond) \(+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})\) (b) \(2 \mathrm{C}\) (graphite) \(+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})\) (c) \(2 \mathrm{C}\) (diamond) \(+4 \mathrm{H}(\mathrm{g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})\) (d) \(2 \mathrm{C}\) (graphite) \(+4 \mathrm{H}(\mathrm{g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})\)

The standard heat of combustion of \(\mathrm{Al}\) is \(-837.8 \mathrm{~kJ}\) \(\mathrm{mol}^{-1}\) at \(25^{\circ} \mathrm{C}\). If \(\mathrm{Al}\) reacts with \(\mathrm{O}_{2}\) at \(25^{\circ} \mathrm{C}\), which of the following releases \(250 \mathrm{kcal}\) of heat? (a) the reaction of \(0.312 \mathrm{~mol}\) of \(\mathrm{Al}\) (b) the formation of \(0.624 \mathrm{~mol}\) of \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (c) the reaction of \(0.712 \mathrm{~mol}\) of \(\mathrm{Al}\) (d) the formation of \(0.615 \mathrm{~mol}\) of \(\mathrm{A} 1 \mathrm{O}_{3}\)

The enthalpy changes for the following processes are listed below. \(\mathrm{Cl}_{2}(\mathrm{~g})=2 \mathrm{C} 1(\mathrm{~g}) ; 242.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\) \(\mathrm{I}_{2}(\mathrm{~g})=21(\mathrm{~g}) ; 151.0 \mathrm{kJmol}^{-1}\) \(\mathrm{ICl}(\mathrm{g})=\mathrm{I}(\mathrm{g})+\mathrm{Cl}(\mathrm{g}) ; 211.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\) \(\mathrm{I}_{2}(\mathrm{~s})=\mathrm{I}_{2}(\mathrm{~g}) ; 62.76 \mathrm{~kJ} \mathrm{~mol}^{-1}\) Given that the standard states for iodine and chlorine are \(\mathrm{I}_{2}\) (s) and \(\mathrm{Cl},(\mathrm{g})\), the standard enthalpy of formation for \(\mathrm{ICl}(\mathrm{g})\) is [2006] (a) \(-14.6 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (b) \(-16.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (c) \(+16.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (d) \(+244.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

Determine \(\Delta \mathrm{H}\) and \(\Delta \mathrm{E}\) for reversible isothermal evaporation of \(90 \mathrm{~g}\) of water at \(100^{\circ} \mathrm{C}\). Assume that water vapour behaves as an ideal gas and heat of evaporation of water is \(540 \mathrm{cal} \mathrm{g}^{-1}\left(\mathrm{R}=2.0 \mathrm{cal} \mathrm{mol}^{-1} \mathrm{~K}^{-1}\right)\) (a) \(48600 \mathrm{cal}, 44870 \mathrm{cal}\) (b) \(43670 \mathrm{cal}, 47700 \mathrm{cal}\) (c) 47700 cal, \(43670 \mathrm{cal}\) (d) \(44870 \mathrm{cal}, 48670 \mathrm{cal}\)

For a reaction at \(300 \mathrm{~K}\), enthalpy and entropy changes are \(-11.5 \times 10^{3} \mathrm{~J} \mathrm{~mol}^{-1}\) and \(-105 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\) respectively. What is the change in Gibbs free energy? (a) \(25 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (b) \(30 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (c) \(15 \mathrm{~kJ} \mathrm{~mol}^{-1}\) (d) \(20 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

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