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Chapter 5: Problem 79

A method of producing phosphine, \(\mathrm{PH}_{3}\), from elemental phosphorus, \(P_{4}\), involves heating the \(P_{4}\) with \(\mathrm{H}_{2} \mathrm{O} .\) An additional product is phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\) Write a balanced equation for this reaction.

Short Answer

Expert verified
The balanced chemical equation for the reaction is \(P_{4} + 6H_{2}O → 4PH_{3} + 4H_{3}PO_{4}\).

Step by step solution

01

Write down the unbalanced chemical equation

First, write down the unbalanced chemical equation from the given information: \(P_{4} + H_{2}O → PH_{3} + H_{3}PO_{4}\)
02

Balance the equation

According to the law of conservation of mass, the amount of atoms that enter a chemical reaction must be equal to the amount of atoms that leave the reaction. Therefore, balance the equation by adjusting the coefficient of each compound so that the number of atoms of each element on the reactant side is equal to the number of atoms of the same element on the product side. The balanced equation is: \(P_{4} + 6H_{2}O → 4PH_{3} + 4H_{3}PO_{4}\).

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Most popular questions from this chapter

Thiosulfate ion, \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\), is a reducing agent that can be oxidized to different products, depending on the strength of the oxidizing agent and other conditions. By adding \(\mathrm{H}^{+}, \mathrm{H}_{2} \mathrm{O},\) and/or \(\mathrm{OH}^{-}\) as necessary, write redox equations to show the oxidation of \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) to (a) \(\mathrm{S}_{4} \mathrm{O}_{6}^{2-}\) by \(\mathrm{I}_{2}\) (iodide ion is another product) (b) \(\mathrm{HSO}_{4}^{-}\) by \(\mathrm{Cl}_{2}\) (chloride ion is another product) (c) \(\mathrm{SO}_{4}^{2-}\) by \(\mathrm{OCl}^{-}\) in basic solution (chloride ion is another product)

Which solution has the greatest \(\left[\mathrm{SO}_{4}^{2-}\right]:\) (a) \(0.075 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4} ; \quad\) (b) \(\quad 0.22 \mathrm{M} \mathrm{MgSO}_{4} ; \quad\) (c) \(\quad 0.15 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\) (d) \(0.080 \mathrm{M} \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} ;\) (e) \(0.20 \mathrm{M} \mathrm{CuSO}_{4} ?\)

A neutralization reaction between an acid and a base is a common method of preparing useful salts. Give net ionic equations showing how the following salts could be prepared in this way: (a) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4};\) (b) \(\mathrm{NH}_{4} \mathrm{NO}_{3} ;\) and \((\mathrm{c})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\).

Explain the important distinctions between (a) a strong electrolyte and strong acid; (b) an oxidizing agent and reducing agent; (c) precipitation reactions and neutralization reactions; (d) half-reaction and overall reaction.

Complete and balance these half-equations. (a) \(\mathrm{SO}_{3}^{2-} \longrightarrow \mathrm{S}_{2} \mathrm{O}_{3}^{2-}\) (acidic solution) (b) \(\mathrm{HNO}_{3} \longrightarrow \mathrm{N}_{2} \mathrm{O}(\mathrm{g})\) (acidic solution) (c) \(\mathrm{Al}(\mathrm{s}) \longrightarrow \mathrm{Al}(\mathrm{OH})_{4}^{-}\) (basic solution) Indicate whether oxidation or reduction is involved.
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