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Chapter 6: Problem 19

The equation for the fermentation of glucose to alcohol and carbon dioxide is: $$ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(a q) \longrightarrow 2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q)+2 \mathrm{CO}_{2}(g) $$ The enthalpy change for the reaction is \(-67 \mathrm{kJ} .\) Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?

Short Answer

Expert verified
The fermentation of glucose to alcohol and carbon dioxide is an exothermic reaction, as the enthalpy change is -67 kJ (negative value). Therefore, energy in the form of heat is evolved, not absorbed, during the reaction.

Step by step solution

01

Understand Exothermic and Endothermic Reactions

Exothermic reactions are chemical reactions that release energy in the form of heat. The enthalpy change for exothermic reactions is negative, as the products have lower energy than the reactants. On the other hand, endothermic reactions are chemical reactions that absorb energy in the form of heat. The enthalpy change for endothermic reactions is positive, as the products have higher energy than the reactants.
02

Determine if the Reaction is Exothermic or Endothermic

As given, the enthalpy change for the fermentation of glucose to alcohol and carbon dioxide is -67 kJ. Since the enthalpy change is negative, it indicates that the reaction is an exothermic reaction.
03

Determine if Heat is Absorbed or Evolved

Since the reaction is exothermic, energy in the form of heat is released during the reaction. Hence, heat is evolved as the reaction occurs. To sum up: 1. The fermentation of glucose to alcohol and carbon dioxide is an exothermic reaction, given its negative enthalpy change. 2. Energy in the form of heat is evolved, not absorbed, as the reaction occurs.

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Most popular questions from this chapter

A serving size of six cookies contains 4 g of fat, 20 of carbohydrates, and 2 g of protein. If walking 1.0 mile consumes 170 kJ of energy, how many miles must you walk to burn off enough calories to eat six cookies? Assume the energy content of fats, carbohydrates, and proteins are 8 kcallg, 4 kcallg, and 4 kcallg, respectively.

Consider a balloon filled with helium at the following conditions. $$ \begin{array}{l}{313 \mathrm{g} \mathrm{He}} \\ {1.00 \mathrm{atm}} \\ {1910 . \mathrm{L}} \\ {\text { Molar Heat Capacity }=20.8 \mathrm{J} / \mathrm{C} \cdot \mathrm{mol}}\end{array} $$ The temperature of this balloon is decreased by \(41.6^{\circ} \mathrm{C}\) as the volume decreases to \(1643 \mathrm{L},\) with the pressure remaining constant. Determine \(q, w,\) and $\Delta E(\text { in } \mathrm{kJ} \text { ) for the compression of }$ the balloon.

Calculate \(\Delta E\) for each of the following. a. \(q=-47 \mathrm{kJ}, w=+88 \mathrm{kJ}\) b. \(q=+82 \mathrm{kJ}, w=-47 \mathrm{kJ}\) c. \(q=+47 \mathrm{kJ}, w=0\) d. In which of these cases do the surroundings do work on the system?

In a coffee-cup calorimeter, 50.0 \(\mathrm{mL}\) of 0.100\(M \mathrm{AgNO}_{3}\) and 50.0 \(\mathrm{mL}\) of 0.100 \(\mathrm{M} \mathrm{HCl}\) are mixed to yield the following reaction: $$\mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{AgCl}(s)$$ The two solutions were initially at \(22.60^{\circ} \mathrm{C}\) , and the final temperature is \(23.40^{\circ} \mathrm{C}\) Calculate the heat that accompanies this reacture in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 100.0 \(\mathrm{g}\) and a specific heat capacity of 4.18 \(\mathrm{J} / \rho \mathrm{C} \cdot \mathrm{g} .\)

Consider the following equations: $$ \begin{array}{ll}{3 \mathrm{A}+6 \mathrm{B} \longrightarrow 3 \mathrm{D}} & {\Delta H=-403 \mathrm{kJ} / \mathrm{mol}} \\ {\mathrm{E}+2 \mathrm{F} \longrightarrow \mathrm{A}} & {\Delta H=-105.2 \mathrm{kJ} / \mathrm{mol}} \\\ {\mathrm{C} \longrightarrow \mathrm{E}+3 \mathrm{D}} & {\Delta H=64.8 \mathrm{kJ} / \mathrm{mol}}\end{array} $$ Suppose the first equation is reversed and multiplied by \(\frac{1}{6},\) the second and third equations are divided by \(2,\) and the three adjusted equations are added. What is the net reaction and what is the overall heat of this reaction?
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