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Chapter 22: Problem 61

Hydrogen peroxide can be prepared by treating barium peroxide with sulfuric acid. Write a balanced equation for this reaction.

Short Answer

Expert verified
The balanced chemical equation for the reaction between barium peroxide and sulfuric acid is: \[BaO2 + 2H2SO4 \rightarrow BaSO4 + 2H2O2\]

Step by step solution

01

Write the Unbalanced Chemical Equation

Start by writing down the chemical reaction. The reaction is between hydrogen peroxide (BaO2) and sulfuric acid (H2SO4) which produces barium sulfate (BaSO4) and hydrogen peroxide (H2O2). So the unbalanced chemical equation will look like this: \[BaO2 + H2SO4 \rightarrow BaSO4 + H2O2\]
02

Balance the Chemical Equation

Looking at the unbalanced equation, it is clear that the hydrogen (H) and oxygen (O) are not balanced. There are two hydrogen atoms on the left-hand side, but there are four on the right (two each in the BaSO4 and the H2O2). Similarly, there are six oxygen atoms on the left (four in the BaO2, two in the H2SO4), but only five on the right (four in the BaSO4, one in the H2O2). To balance the equation, add a coefficient of 2 in front of H2SO4 and H2O2. The balanced equation is: \[BaO2 + 2H2SO4 \rightarrow BaSO4 + 2H2O2\] This increases the amount of hydrogen and oxygen on the left-hand side to match the right-hand side. On both sides, there are now two barium atoms, four hydrogen atoms, and six oxygen atoms.

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Most popular questions from this chapter

Explain why (a) \(\mathrm{NH}_{3}\) is more basic than \(\mathrm{PH}_{3}\) (b) \(\mathrm{NH}_{3}\) has a higher boiling point than \(\mathrm{PH}_{3}\), (c) \(\mathrm{PCl}_{5}\) exists but \(\mathrm{NCl}_{5}\) does not, \((\mathrm{d}) \mathrm{N}_{2}\) is more inert than \(\mathrm{P}_{4}\).

Write a balanced equation for each of the following reactions: (a) Heating phosphorous acid yields phosphoric acid and phosphine \(\left(\mathrm{PH}_{3}\right) .\) (b) Lithium carbide reacts with hydrochloric acid to give lithium chloride and methane. (c) Bubbling HI gas through an aqueous solution of \(\mathrm{HNO}_{2}\) yields molecular iodine and nitric oxide. (d) Hydrogen sulfide is oxidized by chlorine to give \(\mathrm{HCl}\) and \(\mathrm{SCl}_{2}\).

Write a balanced equation for each of the following processes: (a) On heating, ammonium nitrate produces nitrous oxide. (b) On heating, potassium nitrate produces potassium nitrite and oxygen gas. (c) On heating, lead nitrate produces lead(II) oxide, nitrogen dioxide \(\left(\mathrm{NO}_{2}\right),\) and oxygen gas.

Two solutions are labeled A and B. Solution A contains \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and solution \(\mathrm{B}\) contains \(\mathrm{NaHCO}_{3}\). Describe how you would distinguish between the two solutions if you were provided with a \(\mathrm{MgCl}_{2}\) solution. (Hint: You need to know the solubilities of \(\mathrm{MgCO}_{3}\) and \(\mathrm{MgHCO}_{3}\).)

Elements number 17 and 20 form compounds with hydrogen. Write the formulas for these two compounds and compare their chemical behavior in water.
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