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Chapter 3: Problem 13

Balance the following equations: (a) $\mathrm{CaS}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{HS})_{2}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q)$ (b) $\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g)$ (c) $\mathrm{FeCl}_{3}(s)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow \mathrm{Fe}_{2}\left(\mathrm{CO}_{3}\right)_{3}(s)+\mathrm{NaCl}(a q)$ (d) $\mathrm{FeS}_{2}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{SO}_{2}(g)$

Short Answer

Expert verified
(a) \(2\mathrm{CaS}(s) + 3\mathrm{H}_2\mathrm{O}(l) \rightarrow 1\mathrm{Ca}(\mathrm{HS})_2(aq) + 1\mathrm{Ca}(\mathrm{OH})_2(aq)\) (b) \(4\mathrm{NH}_3(g) + 5\mathrm{O}_2(g) \rightarrow 4\mathrm{NO}(g) + 6\mathrm{H}_2\mathrm{O}(g)\)

Step by step solution

01

Begin by counting the number of atoms for each element on both sides of the equation. On the left side, there is 1 \(\mathrm{Ca}\), 1 \(\mathrm{S}\), and 2 \(\mathrm{H}\) and 1 \(\mathrm{O}\). On the right side, there are 2 \(\mathrm{Ca}\), 3 \(\mathrm{H}\), 2 \(\mathrm{S}\), and 2 \(\mathrm{O}\). Step 2: Balance Calcium

On the left side of the equation, add a 2 as the coefficient for \(\mathrm{CaS}\) to balance Calcium. Now, there are 2 \(\mathrm{Ca}\), 2 \(\mathrm{S}\), and 2 \(\mathrm{H}\) and 1 \(\mathrm{O}\) on the left side of the equation. Step 3: Balance Hydrogen
02

Add a 3 as the coefficient for \(\mathrm{H}_2\mathrm{O}\) on the left side to balance Hydrogen. Now, there are 2 \(\mathrm{Ca}\), 2 \(\mathrm{S}\), 6 \(\mathrm{H}\), and 3 \(\mathrm{O}\) on the left side of the equation. Step 4: Balance Final Equation

By comparing all the elements, the balanced equation is: \(2\mathrm{CaS}(s) + 3\mathrm{H}_2\mathrm{O}(l) \rightarrow 1\mathrm{Ca}(\mathrm{HS})_2(aq) + 1\mathrm{Ca}(\mathrm{OH})_2(aq)\) (b) Balancing the reaction: \(\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) Step 1: Count Atoms
03

On the left side, there is 1 \(\mathrm{N}\), 3 \(\mathrm{H}\), and 2 \(\mathrm{O}\). On the right side, there is 1 \(\mathrm{N}\), 2 \(\mathrm{H}\), and 3 \(\mathrm{O}\). Step 2: Balance Nitrogen

Add a 2 as the coefficient for \(\mathrm{NH}_3\) on the left side and \(\mathrm{NO}\) on the right side to balance the Nitrogen. Now, there are 2 \(\mathrm{N}\), 6 \(\mathrm{H}\), and 2 \(\mathrm{O}\) on the left side of the equation. Step 3: Balance Hydrogen
04

Put a 3 as the coefficient for \(\mathrm{H}_2\mathrm{O}\) on the right side to balance Hydrogen. Now, there are 2 \(\mathrm{N}\), 6 \(\mathrm{H}\), and 2 \(\mathrm{O}\) on the left side and 2 \(\mathrm{N}\), 6 \(\mathrm{H}\), and 6 \(\mathrm{O}\) on the right side. Step 4: Balance Final Equation

Finally, balance Oxygen by having 5 \(\mathrm{O}_{2}\) on the left side of the equation, which gives us: \(4\mathrm{NH}_3(g) + 5\mathrm{O}_2(g) \rightarrow 4\mathrm{NO}(g) + 6\mathrm{H}_2\mathrm{O}(g)\)

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Most popular questions from this chapter

When a mixture of \(10.0 \mathrm{~g}\) of acetylene $\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\( and \)10.0 \mathrm{~g}$ of oxygen \(\left(\mathrm{O}_{2}\right)\) is ignited, the resulting combustion reaction produces \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) (a) Write the balanced chemical equation for this reaction. (b) Which is the limiting reactant? (c) How many grams of $\mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{O}_{2}, \mathrm{CO}_{2},\( and \)\mathrm{H}_{2} \mathrm{O}$ are present after the reaction is complete?

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write the balanced chemical equation for this reaction. (b) How many grams of aluminum hydroxide are obtained from \(14.2 \mathrm{~g}\) of aluminum sulfide?

(a) Ibuprofen is a common over-the-counter analgesic with the formula \(\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2} .\) How many moles of \(\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2}\) are in a 500-mg tablet of ibuprofen? Assume the tablet is composed entirely of ibuprofen. (b) How many molecules of $\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2}$ are in this tablet? (c) How many oxygen atoms are in the tablet?

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 \(59.0 \%\) C, \(7.1 \%\) H, \(26.2 \%\) O, and $7.7 \% \mathrm{~N}\( by mass; its molar mass is about \)180 \mathrm{u}$.

An iron ore sample contains \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) together with other substances. Reaction of the ore with CO produces iron metal: $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) $$ (a) Balance this equation. (b) Calculate the number of grams of CO that can react with $0.350 \mathrm{~kg}\( of \)\mathrm{Fe}_{2} \mathrm{O}_{3}$ (c) Calculate the number of grams of Fe and the number of grams of \(\mathrm{CO}_{2}\) formed when \(0.350 \mathrm{~kg}\) of $\mathrm{Fe}_{2} \mathrm{O}_{3}$ reacts. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.
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