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Chapter 19: Problem 30

Write a balanced equation describing the reaction of aluminum metal with concentrated aqueous sodium hydroxide.

Short Answer

Expert verified
The balanced equation for the reaction of aluminum metal with concentrated aqueous sodium hydroxide is: \(2Al(s) + 6NaOH(aq) \rightarrow 2Al(OH)_3(s) + 6Na\)

Step by step solution

01

Determine the products

The reaction between aluminum and sodium hydroxide will result in the formation of aluminum hydroxide and sodium metal. The chemical formulas for these compounds are Al(OH)₃ and Na, respectively.
02

Write the unbalanced chemical equation

Incorporating the reactants and products, the unbalanced equation is: Al(`s) + NaOH(`aq) → Al(OH)₃(s) + Na
03

Balance the chemical equation

To balance the equation, we need to make sure that there are equal numbers of each element on both sides of the equation. The unbalanced equation is: Al(`s) + NaOH(`aq) → Al(OH)₃(s) + Na To balance it, we can start with the aluminum (Al) and hydroxide (OH) ions first. 2Al(`s) + 6NaOH(`aq) → 2Al(OH)₃(s) + 6Na Now the equation is balanced with equal numbers of aluminum, sodium and hydroxide ions on both sides. The balanced equation for the reaction of aluminum metal with concentrated aqueous sodium hydroxide is: 2Al(`s) + 6NaOH(`aq) → 2Al(OH)₃(s) + 6Na

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Most popular questions from this chapter

Which of the following statement(s) is(are) true? a. The alkali metals are found in the earth's crust in the form of pure elements. b. Gallium has one of the highest melting points known for metals. c. When calcium metal reacts with water, one of the products is \(\mathrm{H}_{2}(\mathrm{~g})\) d. When \(\mathrm{AlCl}_{3}\) is dissolved in water, it produces an acidic solution. e. Lithium reacts in the presence of excess oxygen gas to form lithium superoxide.

The oxyanion of nitrogen in which it has the highest oxidation state is the nitrate ion \(\left(\mathrm{NO}_{3}^{-}\right) .\) The corresponding oxyanion of phosphorus is \(\mathrm{PO}_{4}^{3-} .\) The \(\mathrm{NO}_{4}^{3-}\) ion is known but not very stable. The \(\mathrm{PO}_{3}^{-}\) ion is not known. Account for these differences in terms of the bonding in the four anions.

Write a balanced equation describing the reduction of \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) by \(\mathrm{SO}_{2}\) to produce selenium.

The atmosphere contains \(9.0 \times 10^{-6 \%}\) Xe by volume at \(1.0 \mathrm{~atm}\) and \(25^{\circ} \mathrm{C}\) a. Calculate the mass of Xe in a room \(7.26 \mathrm{~m}\) by \(8.80 \mathrm{~m}\) by \(5.67 \mathrm{~m}\) b. A typical person takes in about \(2 \mathrm{~L}\) of air during a breath. How many Xe atoms are inhaled in each breath?

What is a disproportionation reaction? Use the following reduction potentials $$\begin{array}{ll} \mathrm{ClO}_{3}^{-}+3 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{HClO}_{2}+\mathrm{H}_{2} \mathrm{O} & \mathscr{C}^{\circ}=1.21 \mathrm{V} \\ \mathrm{HClO}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{HClO}+\mathrm{H}_{2} \mathrm{O} & \mathscr{C}^{\circ}=1.65 \mathrm{V} \end{array}$$ to predict whether \(\mathrm{HClO}_{2}\) will disproportionate.
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