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Chapter 22: Problem 68

Write a balanced equation for each of the following reactions: (a) Burning magnesium metal in a carbon dioxide atmosphere reduces the \(\mathrm{CO}_{2}\) to carbon. (b) \(\mathrm{In}\) photosynthesis, solar energy is used to produce glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) and \(\mathrm{O}_{2}\) from carbon dioxide and water. (c) When carbonate salts dissolve in water, they produce basic solutions.

Short Answer

Expert verified
(a) Mg + CO2 -> MgO + C (b) 6CO2 + 6H2O -> C6H12O6 + 6O2 (c) MCO3 -> M(OH)2 + CO2

Step by step solution

01

Write the unbalanced equation.

Write down the reactants and products for the given reaction: Mg + CO2 -> MgO + C
02

Balance the equation.

We need to make sure there is the same number of each element on both sides of the equation. To balance the equation, we can multiply any of the compounds by some coefficients. The balanced equation is: Mg + CO2 -> MgO + C For reaction (b):
03

Write the unbalanced equation.

Write down the reactants and products for the given reaction: CO2 + H2O -> C6H12O6 + O2
04

Balance the equation.

We need to make sure there is the same number of each element on both sides of the equation. To balance the equation, we can multiply any of the compounds by some coefficients. The balanced equation is: 6CO2 + 6H2O -> C6H12O6 + 6O2 For reaction (c):
05

Write the general reaction.

Carbonate salts generally dissolve in water and produce hydroxide, or OH- ions. Since the formula of a carbonate salt is MCO3, where M is a metal cation, we can write down the general half-reaction: MCO3 -> MOH + CO2
06

Determine the coefficients.

We need to make sure there is the same number of each element on both sides of the reaction. Considering that the coefficient for the hydroxide ion (OH-) is 2, the balanced half-equation is: MCO3 -> M(OH)2 + CO2 Note that this is a general balanced equation for when carbonate salts dissolve in water and produce basic solutions.

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Most popular questions from this chapter

Nitric acid is a powerful oxidizing agent. Using standard reduction potentials, predict whether the following metals can be oxidized to +2 ions by nitric acid: (a) iron, (b) copper, (c) rhodium, (d) zinc, (e) lead, (f) tin.

Account for the following observations: (a) Phosphorus forms a pentachloride, but nitrogen does not. (b) \(\mathrm{H}_{3} \mathrm{PO}_{2}\) is a monoprotic acid. (c) Phosphonium salts, such as \(\mathrm{PH}_{4} \mathrm{Cl}\), can be formed under anhydrous conditions, but they cannot be made in aqueous solution. (d) White phosphorus is more reactive than red phosphorus.

Which of the following statements are true? (a) Si can form an ion with six fluorine atoms, \(\mathrm{SiF}_{6}^{2-}\), whereas carbon cannot. (b) Si can form three stable compounds containing two \(\mathrm{Si}\) atoms each, \(\mathrm{Si}_{2} \mathrm{H}_{2}, \mathrm{Si}_{2} \mathrm{H}_{4},\) and \(\mathrm{Si}_{2} \mathrm{H}_{6}\) (c) In \(\mathrm{HNO}_{3}\) and \(\mathrm{H}_{3} \mathrm{PO}_{4}\) the central atoms, \(\mathrm{N}\) and \(\mathrm{P}\), have different oxidation states. (d) \(\mathrm{S}\) is more electronegative than Se.

Select the member of group 14 that best fits each description: \((\mathbf{a})\) has the greatest tendency to form multiple bonds with itself, (b) forms polymeric structures with oxygen, (c) is a metal with +2 and +4 oxidation states.

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.
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