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Chapter 3: Problem 15

Write balanced chemical equations corresponding to each of the following descriptions: (a) Potassium cyanide reacts with an aqueous solution of sulfuric acid to form hydrogen cyanide gas. (b) When an aqueous solution of ammonium nitrite \(\left(\mathrm{NH}_{4} \mathrm{NO}_{2}\right)\) reacts with an aqueous solution of potassium hydroxide, ammonia gas, water and metal nitrate is formed. (c) When hydrogen gas is passed over solid hot iron(III) oxide, the resulting reaction produces iron and gaseous water. (d) When liquid ethanoic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) is combusted, carbon dioxide and water are formed.

Short Answer

Expert verified
(a) \(KCN + H_2SO_4 -> HCN + KHSO_4\) (b) \(NH_4NO_2 + KOH -> NH_3 + H_2O + KNO_3\) (c) \(3H_2 + Fe_2O_3 -> 2Fe + 3H_2O\) (d) \(CH_3COOH + 2O_2 -> 2CO_2 + 2H_2O\)

Step by step solution

01

Reaction (a) - Potassium cyanide with sulfuric acid

Firstly, let's write down the chemical formulas of the reactants and products: Reactants: Potassium cyanide (KCN) and sulfuric acid (H2SO4) Product: Hydrogen cyanide gas (HCN) Now let's write the unbalanced chemical equation: KCN + H2SO4 -> HCN Balance the equation by ensuring the same number of each type of atom appears on both sides of the equation: KCN + H2SO4 -> HCN + KHSO4 Our balanced equation is: \(KCN + H_2SO_4 -> HCN + KHSO_4\)
02

Reaction (b) - Ammonium nitrite with potassium hydroxide

Write down the chemical formulas of the reactants and products: Reactants: Ammonium nitrite (NH4NO2) and potassium hydroxide (KOH) Products: Ammonia gas (NH3), water (H2O), and potassium nitrate (KNO3) Now let's write the unbalanced chemical equation: NH4NO2 + KOH -> NH3 + H2O + KNO3 Balance the equation by adjusting the coefficients: NH4NO2 + KOH -> NH3 + H2O + KNO3 Our balanced equation is: \(NH_4NO_2 + KOH -> NH_3 + H_2O + KNO_3\)
03

Reaction (c) - Hydrogen gas with iron(III) oxide

Write down the chemical formulas of the reactants and products: Reactants: Hydrogen gas (H2) and iron(III) oxide (Fe2O3) Products: Iron (Fe) and water (H2O) Now let's write the unbalanced chemical equation: H2 + Fe2O3 -> Fe + H2O Balance the equation by adjusting the coefficients: 3H2 + Fe2O3 -> 2Fe + 3H2O Our balanced equation is: \(3H_2 + Fe_2O_3 -> 2Fe + 3H_2O\)
04

Reaction (d) - Combustion of ethanoic acid

Write down the chemical formulas of the reactants and products: Reactants: Ethanoic acid (CH3COOH) and oxygen gas (O2) Products: Carbon dioxide (CO2) and water (H2O) Now let's write the unbalanced chemical equation: CH3COOH + O2 -> CO2 + H2O Balance the equation by adjusting the coefficients: CH3COOH + 2O2 -> 2CO2 + 2H2O Our balanced equation is: \(CH_3COOH + 2O_2 -> 2CO_2 + 2H_2O\)

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Most popular questions from this chapter

Consider a sample of calcium carbonate in the form of a cube measuring 2.005 in. on each edge. If the sample has a density of $2.71 \mathrm{~g} / \mathrm{cm}^{3},$ how many oxygen atoms does it contain?

Balance the following equations: (a) $\mathrm{SiCl}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Si}(\mathrm{OH})_{4}(s)+\mathrm{HCl}(a q)$ (b) $\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+\mathrm{O}_{2}(g)$ (c) $\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(l) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)$ (d) $\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \longrightarrow \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$

When hydrocarbons are burned in a limited amount of air, both \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\) form. When \(0.450 \mathrm{~g}\) of a particular hydrocarbon was burned in air, \(0.467 \mathrm{~g}\) of $\mathrm{CO}, 0.733 \mathrm{~g}\( of \)\mathrm{CO}_{2},\( and \)0.450 \mathrm{~g}\( of \)\mathrm{H}_{2} \mathrm{O}$ were formed. (a) What is the empirical formula of the compound? (b) How many grams of \(\mathrm{O}_{2}\) were used in the reaction? (c) How many grams would have been required for complete combustion?

The molecular formula of salicylic acid, a compound commonly found in facial cleanser, is \(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\). (a) What is the molar mass of salicylic acid? (b) How many moles of salicylic acid are present in \(0.5 \mathrm{mg}\) of this substance? (c) How many molecules of salicylic acid are in \(0.5 \mathrm{mg}\) of this substance? (d) How many oxygen atoms are present in \(0.5 \mathrm{mg}\) of salicylic acid?

A chemical plant uses electrical energy to decompose aqueous solutions of \(\mathrm{NaCl}\) to give \(\mathrm{Cl}_{2}, \mathrm{H}_{2},\) and \(\mathrm{NaOH}\) : $2 \mathrm{NaCl}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g)$ If the plant produces \(1.5 \times 10^{6} \mathrm{~kg}\) ( 1500 metric tons) of \(\mathrm{Cl}_{2}\) daily, estimate the quantities of \(\mathrm{H}_{2}\) and \(\mathrm{NaOH}\) produced.
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