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Chapter 22: Problem 62

Use information from this chapter and previous chapters to write plausible chemical equations to represent the following: (a) the reaction of silver metal with \(\mathrm{HNO}_{3}(\mathrm{aq})\) (b) the complete combustion of the rocket fuel, unsymmetrical dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\) (c) the preparation of sodium triphosphate by heating a mixture of sodium dihydrogen phosphate and sodium hydrogen phosphate.

Short Answer

Expert verified
The balanced chemical equations are as follows: \n (a) \( 3Ag + 4HNO_{3} \rightarrow 3AgNO_{3} + 2H_{2}O + NO_{2} \) \n (b) \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2} + 3O_{2} \rightarrow 2CO_{2} + 5H_{2}O + N_{2}\) \n (c) \(2NaH_{2}PO_{4} + \mathrm{Na}_{2} \mathrm{HPO}_{4} \rightarrow \mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10} + 2H_{2}O\).

Step by step solution

01

Reaction of Silver with Nitric Acid (HNO3)

The chemical reaction for this follows the pattern of a displacement reaction, where silver displaces hydrogen in nitric acid, resulting in the formation of silver nitrate and water, along with nitrogen dioxide. So, we'll write our reactants: \( Ag + HNO_{3}\), and our products: \(AgNO_{3} + H_{2}O + NO_{2}\). We then balance this equation to get the final relation: \( 3Ag + 4HNO_{3} \rightarrow 3AgNO_{3} + 2H_{2}O + NO_{2} \).
02

Combustion of unsymmetrical dimethylhydrazine

The rocket fueler, unsymmetrical dimethylhydrazine reacts with oxygen from the atmosphere to produce carbon dioxide, water, and nitrogen. The reactants are \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2} + O_{2}\), and the products are \(CO_{2}, H_{2}O, N_{2}\). Balancing the equation, we get \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2} + 3O_{2} \rightarrow 2CO_{2} + 5H_{2}O + N_{2}\).
03

Preparation of Sodium Triphosphate

The reaction involves heating a mixture of sodium dihydrogen phosphate, \(NaH_{2}PO_{4}\), and sodium hydrogen phosphate, \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\), to produce sodium triphosphate, \(\mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10}\), and water. Let's write our reactants \(NaH_{2}PO_{4} + \mathrm{Na}_{2} \mathrm{HPO}_{4}\), and specify the products as \(\mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10} + H_{2}O\). Balancing this gives us the equation: \(2NaH_{2}PO_{4} + \mathrm{Na}_{2} \mathrm{HPO}_{4} \rightarrow \mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10} + 2H_{2}O\).

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Most popular questions from this chapter

When iodine is added to an aqueous solution of iodide ion, the \(I_{3}^{-}\) ion is formed, according to the reaction below: $$\mathrm{I}_{2}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{I}_{3}^{-}(\mathrm{aq})$$ The equilibrium constant for the reaction above is \(K=7.7 \times 10^{2}\) at \(25^{\circ} \mathrm{C}\) (a) What is \(E^{\circ}\) for the reaction above? (b) If a 0.0010 mol sample of \(I_{2}\) is added to 1.0 L of \(0.0050 \mathrm{M} \mathrm{NaI}(\mathrm{aq})\) at \(25^{\circ} \mathrm{C},\) then what fraction of the \(\mathrm{I}_{2}\) remains unreacted at equilibrium?

What is the oxidation state of sulfur in the following compounds? (a) \(\mathrm{S}_{2} \mathrm{Br}_{2}\) (b) \(\mathrm{SCl}_{2}\) (c) \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}_{4} \mathrm{O}_{6}\).

Make a general prediction about which of the halogen elements, \(\mathrm{F}_{2}, \mathrm{Cl}_{2}, \mathrm{Br}_{2},\) or \(\mathrm{I}_{2},\) displaces other halogens from a solution of halide ions. Which of the halogens is able to displace \(\mathrm{O}_{2}(\mathrm{g})\) from water? Which is able to displace \(\mathrm{H}_{2}(\mathrm{g})\) from water?

Suppose that the sulfur present in seawater as \(\mathrm{SO}_{4}^{2-}\) \(\left(2650 \mathrm{mg} \mathrm{L}^{-1}\right)\) could be recovered as elemental sulfur. If this sulfur were then converted to \(\mathrm{H}_{2} \mathrm{SO}_{4},\) how many cubic kilometers of seawater would have to be processed to yield the average U.S. annual consumption of about 45 million tons of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)

Supply an appropriate name for each of the following: (a) \(\mathrm{HPO}_{4}^{2-} ;\) (b) \(\mathrm{Ca}_{2} \mathrm{P}_{2} \mathrm{O}_{7} ;\) (c) \(\mathrm{H}_{6} \mathrm{P}_{4} \mathrm{O}_{13}\).
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