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Chapter 1: Problem 18

Consider the following reaction showing photosynthesis: $$\begin{array}{c}{6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g)} \\ {\Delta H=+2800 \mathrm{kJ} / \mathrm{mol}}\end{array}$$ Which of the following is true regarding the thermal energy in this system? (A) It is transferred from the surroundings to the reaction. (B) It is transferred from the reaction to the surroundings. (C) It is transferred from the reactants to the products. (D) It is transferred from the products to the reactants.

Short Answer

Expert verified
The correct answer is (A) It is transferred from the surroundings to the reaction.

Step by step solution

01

Understanding Endothermic Reactions

In an endothermic reaction, energy or heat is absorbed from the surroundings. In other words, the system (reaction) takes in thermal energy in order for the reaction to proceed. The given reaction is endothermic, as indicated by the positive enthalpy of reaction (\(\Delta H = +2800 \, kJ/mol\)).
02

Applying the Concept

Considering the given options, in an endothermic reaction like the given one, the correct answer would state that the energy transfer takes place from the surroundings to the reaction.
03

Identifying the Correct Option

From the options given, option (A) - 'It is transferred from the surroundings to the reaction' - correctly describes the direction of heat transfer for this endothermic reaction.

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Key Concepts

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

Endothermic Reactions
In the world of chemical reactions, an endothermic reaction stands out due to its unique behavior. During such reactions, energy is not released. Instead, it is absorbed from the environment. This characteristic absorption of energy is essential for the reaction to proceed.
An endothermic reaction can be compared to a person charging a phone with a battery pack. Just as the phone needs to pull in energy to function, an endothermic reaction pulls in energy to occur.
In the photosynthesis reaction depicted, you can observe this phenomena: the reaction takes in energy from the surroundings, thereby maintaining the principle of energy conservation. A positive enthalpy (\(\Delta H = +2800 \, kJ/mol\)) clearly indicates the endothermic nature of this process.
Enthalpy Change
Enthalpy change in a chemical reaction represents the total heat content variation when a reaction occurs. It essentially measures how much heat energy is either absorbed or released.
For the process of photosynthesis, the enthalpy change is positive, suggesting that the reaction absorbs heat. When you see \(\Delta H = +2800 \, kJ/mol\), it signals that for each mole of carbon dioxide and water consumed, 2800 kJ of heat energy is absorbed.
Enthalpy change provides a clear window into the energetic demands of the reaction. Positive enthalpy indicates the need for energy input, as in endothermic reactions, while negative values are observed in exothermic reactions releasing energy.
Thermal Energy Transfer
When discussing chemical reactions, thermal energy transfer is crucial. It explains how energy moves between a system and its surroundings.
In the case of endothermic reactions like photosynthesis, thermal energy is transferred from the surroundings into the system. This process is akin to sunlight warming up the inside of a house through a window. The reaction, just like the house, absorbs and relies on this energy to operate.
This transfer of thermal energy is what enables the conversion of carbon dioxide and water into glucose and oxygen, a fantastic display of nature harnessing energy from its environment to fuel life processes.

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Most popular questions from this chapter

The following reaction is found to be at equilibrium at 25掳C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) What is the expression for the equilibrium constant, \(K_{\mathrm{c}} ?\) (A) \(\frac{\left[\mathrm{SO}_{3}\right]^{2}}{\left[\mathrm{O}_{2}\right]\left[\mathrm{SO}_{2}\right]^{2}}\) (B) \(\frac{2\left[\mathrm{SO}_{3}\right]}{\left[\mathrm{O}_{2}\right] 2\left[\mathrm{SO}_{2}\right]}\) (C) \(\frac{\left[\mathrm{O}_{2}\right]\left[\mathrm{SO}_{2}\right]^{2}}{\left[\mathrm{SO}_{3}\right]^{2}}\) (D) \(\frac{\left[\mathrm{O}_{2}\right] 2\left[\mathrm{SO}_{2}\right]}{2\left[\mathrm{SO}_{3}\right]}\)

The following reaction is found to be at equilibrium at 25掳C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) Which of the following would cause the reverse reaction to speed up? (A) Adding more \(\mathrm{SO}_{3}\) (B) Raising the pressure (C) Lowering the temperature (D) Removing some \(\mathrm{SO}_{2}\)

The following reaction is found to be at equilibrium at 25掳C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) The value for \(K_{\mathrm{c}}\) at \(25^{\circ} \mathrm{C}\) is \(8.1 .\) What must happen in order for the reaction to reach equilibrium if the initial concentrations of all three species was 2.0 \(M\) ? (A) The rate of the forward reactions would increase, and \(\left[\mathrm{SO}_{3}\right]\) would decrease. (B) The rate of the reverse reaction would increase, and \(\left[\mathrm{SO}_{2}\right]\) would decrease. (C) Both the rate of the forward and reverse reactions would increase, and the value for the equilibrium constant would also increase. (D) No change would occur in either the rate of reaction or the concentrations of any of the species.

Questions 32-36 refer to the following. Two half-cells are set up as follows: Half-Cell A: Strip of \(\mathrm{Cu}(s)\) in \(\mathrm{CuNO}_{3}(a q)\) Half-Cell B: Strip of \(\mathrm{Zn}(s)\) in \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\) (aq) When the cells are connected according to the diagram below, the following reaction occurs: GRAPH CAN'T COPY $$2 \mathrm{Cu}^{+}(a q)+\mathrm{Zn}(s) \rightarrow 2 \mathrm{Cu}(s)+\mathrm{Zn}^{2+}(a q) E^{\circ}=+1.28 \mathrm{V}$$ If the \(\mathrm{Cu}^{+}+e^{-} \rightarrow \mathrm{Cu}(s)\) half-reaction has a standard reduction potential of \(+0.52 \mathrm{V},\) what is the standard reduction potential for the \(\mathrm{Zn}^{2+}+2 e^{-} \rightarrow \mathrm{Zn}(s)\) half-reaction? (A) \(+0.76 \mathrm{V}\) (B) \(-0.76 \mathrm{V}\) (C) \(+0.24 \mathrm{V}\) (D) \(-0.24 \mathrm{V}\)

After 44 minutes, a sample of \(_{19}^{44} \mathrm{K}\) is found to have decayed to 25 percent of the original amount present. What is the half-life of \(_{19}^{44} \mathrm{K}?\) (A) 11 minutes (B) 22 minutes (C) 44 minutes (D) 66 minutes
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