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Chapter 3: Problem 16

Write balanced chemical equations to correspond to each of the following descriptions: (a) When sulfur trioxide gas reacts with water, a solution of sulfuric acid forms. b) Boron sulfide, \(\mathrm{B}_{2} \mathrm{~S}_{3}(s)\), reacts violently with water to form dissolved boric acid, \(\mathrm{H}_{3} \mathrm{BO}_{3}\), and hydrogen sulfide gas. (c) Phosphine, \(\mathrm{PH}_{3}(g)\), combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide. (d) When solid mercury(II) nitrate is heated, it decomposes to form solid mercury(II) oxide, gaseous nitrogen dioxide, and oxygen. (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.

Short Answer

Expert verified
The balanced chemical equations are as follows: (a) SO鈧(g) + H鈧侽(l) 鈫 H鈧係O鈧(aq) (b) B鈧係鈧(s) + 6H鈧侽(l) 鈫 2H鈧傿O鈧(aq) + 3H鈧係(g) (c) 4PH鈧(g) + 5O鈧(g) 鈫 6H鈧侽(g) + P鈧凮鈧佲個(s) (d) 2Hg(NO鈧)鈧(s) 鈫 2HgO(s) + 4NO鈧(g) + O鈧(g) (e) Cu(s) + H鈧係O鈧(aq) 鈫 CuSO鈧(aq) + SO鈧(g) + H鈧侽(l)

Step by step solution

01

Identify reactants and products, and write their chemical formulas

Reactants: Sulfur trioxide (SO鈧), water (H鈧侽) Product: Sulfuric acid (H鈧係O鈧)
02

Write the unbalanced chemical equation

SO鈧(g) + H鈧侽(l) 鈫 H鈧係O鈧(aq)
03

Balance the equation

SO鈧(g) + H鈧侽(l) 鈫 H鈧係O鈧(aq) (Already balanced) (b) Boron sulfide, B鈧係鈧(s), reacts violently with water to form dissolved boric acid, H鈧傿O鈧, and hydrogen sulfide gas.
04

Identify reactants and products, and write their chemical formulas

Reactants: Boron sulfide (B鈧係鈧), water (H鈧侽) Products: Boric acid (H鈧傿O鈧), hydrogen sulfide (H鈧係)
05

Write the unbalanced chemical equation

B鈧係鈧(s) + H鈧侽(l) 鈫 H鈧傿O鈧(aq) + H鈧係(g)
06

Balance the equation

B鈧係鈧(s) + 6H鈧侽(l) 鈫 2H鈧傿O鈧(aq) + 3H鈧係(g) (c) Phosphine, PH鈧(g), combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide.
07

Identify reactants and products, and write their chemical formulas

Reactants: Phosphine (PH鈧), oxygen (O鈧) Products: Water vapor (H鈧侽), tetraphosphorus decaoxide (P鈧凮鈧佲個)
08

Write the unbalanced chemical equation

PH鈧(g) + O鈧(g) 鈫 H鈧侽(g) + P鈧凮鈧佲個(s)
09

Balance the equation

4PH鈧(g) + 5O鈧(g) 鈫 6H鈧侽(g) + P鈧凮鈧佲個(s) (d) When solid mercury(II) nitrate is heated, it decomposes to form solid mercury(II) oxide, gaseous nitrogen dioxide, and oxygen.
10

Identify reactants and products, and write their chemical formulas

Reactant: Mercury(II) nitrate (Hg(NO鈧)鈧) Products: Mercury(II) oxide (HgO), nitrogen dioxide (NO鈧), oxygen (O鈧)
11

Write the unbalanced chemical equation

Hg(NO鈧)鈧(s) 鈫 HgO(s) + NO鈧(g) + O鈧(g)
12

Balance the equation

2Hg(NO鈧)鈧(s) 鈫 2HgO(s) + 4NO鈧(g) + O鈧(g) (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.
13

Identify reactants and products, and write their chemical formulas

Reactants: Copper (Cu), sulfuric acid (H鈧係O鈧) Products: Copper(II) sulfate (CuSO鈧), sulfur dioxide (SO鈧), water (H鈧侽)
14

Write the unbalanced chemical equation

Cu(s) + H鈧係O鈧(aq) 鈫 CuSO鈧(aq) + SO鈧(g) + H鈧侽(l)
15

Balance the equation

Cu(s) + H鈧係O鈧(aq) 鈫 CuSO鈧(aq) + SO鈧(g) + H鈧侽(l) (Already balanced)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Reactions
Chemical reactions are processes where substances, called reactants, change into new substances, known as products. This transformation occurs due to the rearrangement of atoms, creating a new set of chemical bonds in the products.
In the world of chemistry, these reactions are represented using chemical equations, which show the essential details of the reactants converting into products. Observing these transformations allows us to understand how substances interact and how new compounds form.
For instance, when sulfur trioxide reacts with water to form sulfuric acid, a chemical reaction occurs. Reactants on the left side of the chemical equation, like sulfur trioxide (\( ext{SO}_3(g) \)) and water (\( ext{H}_2 ext{O}(l) \)), come together to produce a new compound, such as sulfuric acid (\( ext{H}_2 ext{SO}_4(aq) \)) which is found on the right side.
Balancing Equations
Balancing chemical equations is crucial because it reflects the conservation of mass principle. This principle ensures that atoms are neither created nor destroyed in a chemical reaction. Consequently, the number of atoms of each element must be the same on both sides of the equation.
Balancing begins with writing the correct unbalanced equation using chemical formulas, outlining what happens during the reaction.
Here's an example: Boron sulfide (\( ext{B}_2 ext{S}_3(s) \)) reacts with water (\( ext{H}_2 ext{O}(l) \)) to form boric acid (\( ext{H}_3 ext{BO}_3(aq) \)) and hydrogen sulfide (\( ext{H}_2 ext{S}(g) \)). To balance the equation, coefficients are used:
  1. Determine the initial amounts of each element on both sides.
  2. Adjust the coefficients to equalize the number of each type of atom in the reactants and products.
  3. Check your work to ensure the equation is balanced.
Thus, the balanced equation becomes (\[ ext{B}_2 ext{S}_3(s) + 6 ext{H}_2 ext{O}(l) \rightarrow 2 ext{H}_3 ext{BO}_3(aq) + 3 ext{H}_2 ext{S}(g) \]).
Reactants and Products
In any chemical equation, reactants and products are fundamental components. Reactants are the starting substances that undergo a chemical change.
Products are the new substances formed as a result of the reaction. The transformation from reactants to products is what defines a chemical reaction.
Understanding the nature and composition of these chemicals is essential. The chemical equations are like recipes that tell us what's needed and what's produced. For example, in this exercise:
  • Reactants, such as phosphine (\( ext{PH}_3(g) \)) and oxygen (\( ext{O}_2(g) \)), start the reaction.
  • Products, like water vapor (\( ext{H}_2 ext{O}(g) \)) and tetraphosphorus decaoxide (\( ext{P}_4 ext{O}_{10}(s) \)), are the outcome of the chemical process.
Accurate identification of reactants and products is crucial for crafting correct and balanced chemical equations.

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Most popular questions from this chapter

Determine the empirical and molecular formulas of each of the following substances: (a) Ibuprofen, a headache remedy, contains \(75.69 \% \mathrm{C}\), \(8.80 \% \mathrm{H}\), and \(15.51 \% \mathrm{O}\) by mass, and has a molar mass of \(206 \mathrm{~g} / \mathrm{mol}\). (b) Cadaverine, a foul-smelling substance produced by the action of bacteria on meat, contains \(58.55 \% \mathrm{C}\), \(13.81 \% \mathrm{H}\), and \(27.40 \% \mathrm{~N}\) by mass; its molar mass is \(102.2 \mathrm{~g} / \mathrm{mol}\) (c) Epinephrine (adrenaline), a hormone secreted into the bloodstream in times of danger or stress, contains \(59.0 \%\) \(\mathrm{C}, 7.1 \% \mathrm{H}, 26.2 \% \mathrm{O}\), and \(7.7 \% \mathrm{~N}\) by mass; its \(\mathrm{MW}\) is about 180 amu.

(a) What scientific principle or law is used in the process of balancing chemical equations? (b) In balancing equations is it acceptable to change the coefficients, the subscripts in the chemical formula, or both?

Automotive air bags inflate when sodium azide, \(\mathrm{NaN}_{3}\), rapidly decomposes to its component elements: $$ 2 \mathrm{NaN}_{3}(s) \longrightarrow 2 \mathrm{Na}(s)+3 \mathrm{~N}_{2}(g) $$ (a) How many moles of \(\mathrm{N}_{2}\) are produced by the decomposition of \(1.50 \mathrm{~mol}\) of \(\mathrm{NaN}_{3}\) ? (b) How many grams of \(\mathrm{NaN}_{3}\) are required to form \(10.0 \mathrm{gg}\) of nitrogen gas? (c) How many grams of \(\mathrm{NaN}_{3}\) are required to produce \(10.0 \mathrm{ft}^{3}\) of nitrogen gas, about the size of an automotive air bag, if the gas has a density of \(1.25 \mathrm{~g} / \mathrm{L}\) ?

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) \(\mathrm{C}_{3} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (b) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (c) \(\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{N}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{NH}_{3}(g)\) (e) \(\mathrm{K}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{KOH}(a q)\)

Write a balanced chemical equation for the reaction that occurs when (a) titanium metal undergoes a combination reaction with \(\mathrm{O}_{2}(g) ;\) (b) silver(I) oxide decomposes into silver metal and oxygen gas when heated; (c) propanol, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(l)\) burns in air; (d) methyl tert-butyl ether, \(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{O}(l)\), burns in air.
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