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Chapter 14: Problem 102

Photosynthesis can be represented by $$\begin{array}{r}6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \\\\\Delta H^{\circ}=2801 \mathrm{~kJ} / \mathrm{mol}\end{array}$$ Explain how the equilibrium would be affected by the following changes: (a) Partial pressure of \(\mathrm{CO}_{2}\) is increased. (b) \(\mathrm{O}_{2}\) is removed from the mixture. (c) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (glucose) is removed from the mixture. (d) More water is added. (e) A catalyst is added. (f) Temperature is decreased.

Short Answer

Expert verified
(a) The reaction shifts to the right to decrease CO2. (b) The reaction shifts to the right to produce O2. (c) The reaction shifts to the right to reproduce glucose. (d) The equilibrium shifts to the right to balance the increased water. (e) The catalyst does not alter the equilibrium position. (f) Lower temperature shifts equilibrium to the left.

Step by step solution

01

Determine impact of increased CO2

If the partial pressure of CO2 is increased, the equilibrium would shift to the right according to Le Chatelier's principle. The system stabilizes the increase in CO2 by creating more glucose and oxygen, thereby reducing the amount of excess CO2.
02

Discuss removal of O2

If O2 is removed from the mixture, the equilibrium shifts to the right, again as per Le Chatelier's principle. By eliminating O2, the reaction can compensate by producing more O2 and glucose from CO2 and water.
03

Explain effect of removing glucose

If glucose is removed from the system, the equilibrium would shift to the right. The reaction compensates for the absence of glucose by producing more of it from CO2 and water.
04

Determine influence of adding water

Adding more water to the mixture causes the reaction to shift to the right. This is because, to balance the concentration, the reaction produces additional glucose and oxygen.
05

Discuss impact of adding a catalyst

Adding a catalyst doesn't affect the position of the equilibrium. It only speeds up the rate at which the equilibrium is achieved.
06

Explain effect of decreasing temperature

As photosynthesis is an endothermic reaction (absorbs heat, positive delta H), lowering the temperature would shift the equilibrium to the left, and less glucose and oxygen would be produced as the system tries to counteract the temperature drop by generating heat.

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Most popular questions from this chapter

When a gas was heated under atmospheric conditions, its color deepened. Heating above \(150^{\circ} \mathrm{C}\) caused the color to fade, and at \(550^{\circ} \mathrm{C}\) the color was barely detectable. However, at \(550^{\circ} \mathrm{C},\) the color was partially restored by increasing the pressure of the system. Which of the following best fits the above description? Justify your choice. (a) A mixture of hydrogen and bromine, (b) pure bromine, (c) a mixture of nitrogen dioxide and dinitrogen tetroxide. (Hint: Bromine has a reddish color and nitrogen dioxide is a brown gas. The other gases are colorless.)

Heating solid sodium bicarbonate in a closed vessel establishes the following equilibrium: $$2 \mathrm{NaHCO}_{3}(s) \rightleftharpoons \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}_{2}(g)$$ What would happen to the equilibrium position if (a) some of the \(\mathrm{CO}_{2}\) were removed from the system; (b) some solid \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) were added to the system; (c) some of the solid \(\mathrm{NaHCO}_{3}\) were removed from the system? The temperature remains constant.

Define homogeneous equilibrium and heterogeneous equilibrium. Give two examples of each.

Write equilibrium constant expressions for \(K_{\mathrm{c}},\) and for \(K_{P}\), if applicable, for the following processes: (a) \(2 \mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g)\) (b) \(3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{O}_{3}(g)\) (c) \(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g)\) (d) \(\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{C}(s) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) (e) \(\mathrm{HCOOH}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{HCOO}^{-}(a q)\) (f) \(2 \mathrm{HgO}(s) \rightleftharpoons 2 \mathrm{Hg}(l)+\mathrm{O}_{2}(g)\)

What effect does an increase in pressure have on each of the following systems at equilibrium? The temperature is kept constant and, in each case, the reactants are in a cylinder fitted with a movable piston. (a) \(\mathrm{A}(s) \rightleftharpoons 2 \mathrm{~B}(s)\) (b) \(2 \mathrm{~A}(l) \rightleftharpoons \mathrm{B}(l)\) (c) \(\mathrm{A}(s) \rightleftharpoons \mathrm{B}(g)\) (d) \(\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)\) (e) \(\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)\)
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