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Chapter 22: Problem 48

Explain why, under normal conditions, the reaction of zinc with nitric acid does not produce hydrogen.

Short Answer

Expert verified
Under normal conditions, the reaction of zinc with nitric acid doesn't produce hydrogen due to nitric acid's strong oxidising property. It oxidizes the hydrogen ions into water immediately, preventing the formation of hydrogen gas, and gets reduced in the process.

Step by step solution

01

Understand reactants

Zinc is a metal, and, in most cases, when a metal reacts with an acid, hydrogen gas is produced. Nitric acid, however, behaves differently compared to other typical acids because it's a strong oxidising agent.
02

Understand the reaction

Due to its oxidising properties, nitric acid doesn't just donate a proton (which is what acids typically do), but also brings about oxidation. If zinc was to lose electrons (oxidation), which is what usually happens when metals react with an acid, these electrons would be removed by the nitric acid due to its strong oxidising nature. This prevents any hydrogen gas from being formed because the hydrogen ions are immediately oxidized by the nitric acid to water.
03

Express the reaction

The overall reaction can be represented using the following balance chemical equation: \(Zn(s) + 2HNO_3(aq) \rightarrow Zn(NO_3)_2(aq) + H_2 O(l)\). The nitric acid is being reduced by the zinc, and in the process, it forms water, hence no hydrogen gas is produced.

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Most popular questions from this chapter

What is the change in oxidation number for the following reaction? $$3 \mathrm{O}_{2} \longrightarrow 2 \mathrm{O}_{3}$$

(a) Which of the following compounds has the greatest ionic character: \(\mathrm{PCl}_{5}, \mathrm{SiCl}_{4}, \mathrm{CCl}_{4}, \mathrm{BCl}_{3} ?\) (b) Which of the following ions has the smallest ionic radius: \(\mathrm{F}^{-}, \mathrm{C}^{4-}, \mathrm{N}^{3-}, \mathrm{O}^{2-} ?(\mathrm{c})\) Which of the following atoms has the highest ionization energy: \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I} ?(\mathrm{~d})\) Which of the following oxides is most acidic: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{SiO}_{2}, \mathrm{CO}_{2} ?\)

Describe what is meant by the "hydrogen economy."

Hydrogen peroxide is unstable and decomposes readily: $$2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)$$ This reaction is accelerated by light, heat, or a catalyst. (a) Explain why hydrogen peroxide sold in drugstores comes in dark bottles. (b) The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from \(15.0 \mathrm{~g}\) of a 7.50 percent hydrogen peroxide solution?

Consider the reaction $$\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$$ Given that the \(\Delta G^{\circ}\) for the reaction at \(298 \mathrm{~K}\) is \(173.4 \mathrm{~kJ} / \mathrm{mol},\) calculate (a) the standard free energy of formation of \(\mathrm{NO},\) (b) \(K_{P}\) for the reaction, \((\mathrm{c}) K_{\mathrm{c}}\) for the reaction.
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