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Chapter 4: Problem 64

A plant requires approximately 4178 kcal for the production of \(1.00 \mathrm{kg}\) of starch (Chapter 19 ) from carbon dioxide and water. (a) Is the production of starch in a plant an exothermic process or an endothermic process? (b) Calculate the energy in kilocalories required by a plant for the production of \(6.32 \mathrm{g}\) of starch.

Short Answer

Expert verified
(a) Endothermic process; (b) 26.398 kcal.

Step by step solution

01

Understanding Energy Requirement

The production of starch in plants involves converting carbon dioxide and water into glucose and then to starch using photosynthesis. This process requires energy. Since it needs energy input from sunlight, it is considered an endothermic process.
02

Conversion from Kilograms to Grams

First, we need to convert the mass given in grams to kilograms to match the energy requirement ratio. Since there's 1 kilogram in 1000 grams, we have:\[ 6.32 ext{ g} = 0.00632 ext{ kg} \]
03

Calculate Energy Requirement

Given that the plant requires 4178 kcal to produce 1 kg of starch, we calculate the energy required for 0.00632 kg by setting up a proportion. Thus, the energy required is:\[ 4178 ext{ kcal} imes 0.00632 ext{ kg} = 26.398 ext{ kcal} \]

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Key Concepts

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

Starch Production
In the world of plants, starch production is a crucial part of their growth and energy storage processes. Plants produce starch through the method of photosynthesis. During this process, plants convert sunlight, water, and carbon dioxide into glucose.
Glucose is then polymerized into starch, which plants use as a storage form of energy. Starch can be found in many parts of a plant, most commonly in the roots, seeds, and tubers.
  • The stored energy in starch is critical for plants as it provides them with food that can be broken down and used when sunlight is absent.
  • This process is essential not only for plant survival but also for the life forms that depend on plants for food, including humans.
Understanding starch production helps us appreciate the beautiful complexity of plant biology and the essential role plants play in our ecosystem.
Endothermic Process
Photosynthesis, the process responsible for starch production, is an example of an endothermic process. This means it absorbs energy rather than releasing it.
In photosynthesis, energy from sunlight is captured by chlorophyll in the plant cells. This energy is then used to drive a chemical reaction that converts carbon dioxide and water into glucose and oxygen.
Here are some key points about endothermic processes:
  • Endothermic processes require an input of energy from the environment.
  • In the case of photosynthesis, the energy comes from sunlight, making it an energy-consuming process.
Recognizing photosynthesis as an endothermic process helps us understand why plants need sunlight and how they contribute to the energy balance of our environment.
Energy Calculation in Plants
Energy calculation in plants is essential for understanding how much energy is involved in various biological processes, such as the production of starch. When we say that producing starch requires 4178 kilocalories for each kilogram, we are looking at the energy input needed.
To calculate the energy required for smaller amounts of starch, a simple proportion can be used. For instance, if a plant produces 6.32 grams of starch, we convert that to kilograms to match the energy ratio, which gives us 0.00632 kg.
  • This conversion helps maintain consistency when applying the energy calculation.
  • The proportion is then used to determine the precise energy needed for the 6.32 grams, which results in 26.398 kilocalories.
This calculation is crucial for biologists and agriculturists who need to predict and analyze plant growth and energy needs in various contexts.

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Most popular questions from this chapter

A solar cell generates \(500 .\) k.J of energy per hour. To keep a refrigerator at \(4^{\circ} \mathrm{C}\), one needs \(250 . \mathrm{kcal} / \mathrm{h}\). Can the solar cell supply sufficient energy per hour to maintain the temperature of the refrigerator?

A typical deposit of cholesterol, \(\mathrm{C}_{27} \mathrm{H}_{46} \mathrm{O}\), in an artery might have a mass of 3.9 mg. How many molecules of cholesterol are in this mass?

Answer true or false. (a) When a substance is oxidized, it loses electrons. (b) When a substance gains electrons, it is reduced. (c) In a redox reaction, the oxidizing agent becomes reduced. (d) In a redox reaction, the reducing reagent becomes oxidized. (e) When Zn is converted to \(\mathrm{Zn}^{2+}\) ion, zinc is oxidized. (f) Oxidation can also be defined as the loss of oxygen atoms and/or the gain of hydrogen atoms. (g) Reduction can also be defined as the gain of oxygen atoms and/or the loss of hydrogen atoms. (h) When oxygen, \(O_{2},\) is converted to hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2},\) we say that \(\mathrm{O}_{2}\) is reduced. (i) Hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\), is an oxidizing agent. (j) All combustion reactions are redox reactions. (k) The products of complete combustion (oxidation) of hydrocarbon fuels are carbon dioxide, water, and heat. (l) In the combustion of hydrocarbon fuels, oxygen is the oxidizing agent and the hydrocarbon fuel is the reducing agent. \((\mathrm{m})\) Incomplete combustion of hydrocarbon fuels can produce significant amounts of carbon monoxide. (n) Most common bleaches are oxidizing agents.

Using the equation: \(\mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{s})+3 \mathrm{CO}(\mathrm{g}) \longrightarrow 2 \mathrm{Fe}(\mathrm{s})+3 \mathrm{CO}_{2}(\mathrm{g})\) (a) Show that this is a redox reaction. Which species is oxidized, and which is reduced? (b) How many moles of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) are required to produce 38.4 mol of \(\mathrm{Fe} ?\) (c) How many grams of CO are required to produce \(38.4 \mathrm{mol}\) of \(\mathrm{Fe} ?\)

When a solution of ammonium chloride is added to a solution of lead(II) nitrate, \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\), a white precipitate, lead(II) chloride, forms. Write a balanced net ionic equation for this reaction. Both ammonium chloride and lead(II) nitrate exist as dissociated ions in aqueous solution.
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