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Chapter 13: Problem 69

Old-fashioned "smelling salts" consist of ammonium carbonate, \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3} .\) The reaction for the decomposition of ammonium carbonate $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(s) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) $$ is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?

Short Answer

Expert verified
As the decomposition of ammonium carbonate is an endothermic reaction, increasing the temperature will shift the equilibrium towards the products. This leads to an increase in the concentration of ammonia (NH3), which in turn increases the smell of ammonia. Therefore, the smell of ammonia will increase as the temperature is increased.

Step by step solution

01

Understand the reaction and Le Chatelier's principle

We are given the decomposition reaction of ammonium carbonate as: \[ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(s) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \] This reaction is endothermic, which means it absorbs heat from the surroundings. According to Le Chatelier's principle, if we increase the temperature in an endothermic reaction, the equilibrium will shift in the direction that absorbs the added heat. In this case, the equilibrium will shift towards the products.
02

Determine the effect of increasing temperature

Since the reaction is endothermic, increasing the temperature will lead to a shift in equilibrium towards the products. This is to counteract the increase in temperature by absorbing the heat through the endothermic reaction. As a result, the concentrations of the products (NH3, CO2, and H2O) will increase.
03

Relate the effect to the smell of ammonia

When the concentration of ammonia (NH3) increases, it implies that more ammonia is released as a gas. As the smell of ammonia is due to the presence of ammonia gas, if the concentration increases, it indicates that the smell of ammonia will increase as well. In conclusion, as the temperature is increased in an endothermic reaction like the decomposition of ammonium carbonate, the smell of ammonia will increase.

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Most popular questions from this chapter

At a particular temperature, \(K=2.0 \times 10^{-6}\) for the reaction $$ 2 \mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) $$ If \(2.0 \mathrm{~mol} \mathrm{CO}_{2}\) is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species.

A sample of \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\) is placed in an empty cylinder at \(25^{\circ} \mathrm{C}\). After equilibrium is reached the total pressure is \(1.5\) atm and \(16 \%\) (by moles) of the original \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\) has dissociated to \(\mathrm{NO}_{2}(g)\). a. Calculate the value of \(K_{\mathrm{p}}\) for this dissociation reaction at \(25^{\circ} \mathrm{C}\). b. If the volume of the cylinder is increased until the total pressure is \(1.0 \mathrm{~atm}\) (the temperature of the system remains constant), calculate the equilibrium pressure of \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\) and \(\mathrm{NO}_{2}(g)\). c. What percentage (by moles) of the original \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\) is dissociated at the new equilibrium position (total pressure \(=1.00 \mathrm{~atm}\) )?

Consider the reaction $$ \mathrm{Fe}^{3+}(a q)+\mathrm{SCN}^{-}(a q) \rightleftharpoons \mathrm{FeSCN}^{2+}(a q) $$ How will the equilibrium position shift if a. water is added, doubling the volume? b. \(\mathrm{AgNO}_{3}(a q)\) is added? (AgSCN is insoluble.) c. \(\mathrm{NaOH}(a q)\) is added? \(\left[\mathrm{Fe}(\mathrm{OH})_{3}\right.\) is insoluble.] d. \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) is added?

Peptide decomposition is one of the key processes of digestion, where a peptide bond is broken into an acid group and an amine group. We can describe this reaction as follows: Peptide \((a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons\) acid group \((a q)+\) amine group \((a q)\) If we place \(1.0\) mol peptide into \(1.0 \mathrm{~L}\) water, what will be the equilibrium concentrations of all species in this reaction? Assume the \(K\) value for this reaction is \(3.1 \times 10^{-5}\).

Suppose a reaction has the equilibrium constant \(K=1.7 \times 10^{-8}\) at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
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