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Chapter 22: Problem 65

Complete and balance the following equations: (a) \(\mathrm{ZnCO}_{3}(s) \stackrel{\Delta}{\longrightarrow}\) (b) \(\mathrm{BaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (d) \(\mathrm{CS}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow\) (e) \(\mathrm{Ca}(\mathrm{CN})_{2}(s)+\operatorname{HBr}(a q) \longrightarrow\)

Short Answer

Expert verified
(a) \( ZnCO_3(s) \stackrel{\Delta}{\longrightarrow} ZnO(s) + CO_2(g) \) (b) \( BaC_2(s) + 2 H_2O(l) \longrightarrow Ba(OH)_2(s) + C_2H_2(g) \) (c) \( 2 C_2H_2(g) + 5 O_2(g) \longrightarrow 4 CO_2(g) + 4 H_2O(g) \) (d) \( CS_2(g) + 3 O_2(g) \longrightarrow CO_2(g) + 2 SO_2(g) \) (e) \( Ca(CN)_2(s) + 2 HBr(aq) \longrightarrow CaBr_2(aq) + 2 HCN(aq) \)

Step by step solution

01

Balance equation (a)

(a) ZnCO3(s) → ZnO(s) + CO2(g) Since there is 1 Zn, 1 C, and 3 O atoms on both sides of the equation, it is already balanced.
02

Balance equation (b)

(b) BaC2(s) + H2O(l) → Ba(OH)2(s) + C2H2(g) First, balance the Ba atoms: 1 Ba on both sides, no change needed. Next, balance the C atoms: 2 C on the left, 2 C on the right, no change needed. Finally, balance the H and O atoms by placing a "2" in front of H2O and Ba(OH)2: BaC2(s) + 2 H2O(l) → Ba(OH)2(s) + C2H2(g)
03

Balance equation (c)

(c) C2H2(g) + O2(g) → CO2(g) + H2O(g) First, balance the C atoms by placing a "2" in front of CO2: C2H2(g) + O2(g) → 2 CO2(g) + H2O(g) Next, balance the H atoms by placing a "2" in front of H2O: C2H2(g) + O2(g) → 2 CO2(g) + 2 H2O(g) Finally, balance the O atoms by placing a "5/2" in front of O2 and multiplying all coefficients by 2: 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 4 H2O(g)
04

Balance equation (d)

(d) CS2(g) + O2(g) → CO2(g) + SO2(g) First, balance the C atoms: 1 C on both sides, no change needed. Next, balance the S atoms by placing a "2" in front of SO2: CS2(g) + O2(g) → CO2(g) + 2 SO2(g) Finally, balance the O atoms by placing a "3" in front of O2: CS2(g) + 3 O2(g) → CO2(g) + 2 SO2(g)
05

Balance equation (e)

(e) Ca(CN)2(s) + HBr(aq) → CaBr2(aq) + HCN(aq) First, balance the Ca atoms: 1 Ca on both sides, no change needed. Next, balance the Br atoms by placing a "2" in front of HBr and CaBr2: Ca(CN)2(s) + 2 HBr(aq) → CaBr2(aq) + HCN(aq) Finally, balance the C and N atoms by placing a "2" in front of HCN: Ca(CN)2(s) + 2 HBr(aq) → CaBr2(aq) + 2 HCN(aq)

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Most popular questions from this chapter

(a) The \(\mathrm{P}_{4}, \mathrm{P}_{4} \mathrm{O}_{6}\) and $\mathrm{P}_{4} \mathrm{O}_{10}$ molecules have a common structural feature of four \(\mathrm{P}\) atoms arranged in a tetrahedron (Figures 22.27 and 22.28 ). Does this mean that the bonding between the \(\mathrm{P}\) atoms is the same in all these cases? Explain. (b) Sodium trimetaphosphate $\left(\mathrm{Na}_{3} \mathrm{P}_{3} \mathrm{O}_{9}\right)$ and sodium tetrametaphosphate \(\left(\mathrm{Na}_{4} \mathrm{P}_{4} \mathrm{O}_{12}\right)\) are used as water-softening agents. They contain cyclic $\mathrm{P}_{3} \mathrm{O}_{9}^{3-}\( and \)\mathrm{P}_{4} \mathrm{O}_{12}{ }^{4-}$ ions, respectively. Propose reasonable structures for these ions.

Write a balanced chemical reaction for the condensation reaction between \(\mathrm{H}_{3} \mathrm{PO}_{4}\), molecules to form $\mathrm{H}_{6} \mathrm{P}_{4} \mathrm{O}_{13}$.

One method proposed for removing \(\mathrm{SO}_{2}\) from the flue gases of power plants involves scrubbing with an alkali solid such as calcium carbonate to form calcium sulfite and carbon dioxide gas. (a) Write a balanced chemical equation for the reaction. (b) What mass of \(\mathrm{CaCO}_{3}\) would be required to remove the \(\mathrm{SO}_{2}\) formed by burning \(1000 \mathrm{~kg}\) of coal containing \(8.0 \% \mathrm{~S}\) by mass? (c) What volume of \(\mathrm{CO}_{2}\) is formed under standard temperature and pressure? Assume that all reactions are \(100 \%\) efficient.

Write a balanced equation for each of the following reactions: (a) Sulfur dioxide reacts with water. (b) Solid zinc sulfide reacts with hydrochloric acid. (c) Elemental sulfur reacts with sulfite ion to form thiosulfate. (d) Sulfur trioxide is dissolved in sulfuric acid.

(a) Draw the Lewis structures for at least four species that have the general formula $$[: \mathrm{X} \equiv \mathrm{Y}:]^{n}$$ where \(X\) and Y may be the same or different, and \(n\) may have a value from +1 to \(-2 .\) (b) Which of the compounds is likely to be the strongest Bronsted base? Explain. [Sections 22.1, 22.7, and 22.9]
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