Solved: Relating Gas Variables and Reaction

Chapter , Problem 1PE

(choose chapter or problem)

When silver oxide is heated, it decomposes according to the reaction:

\(2 \mathrm{Ag}_{2} \mathrm{O}(\mathrm{s}) \rightarrow^{\Delta} 4 \mathrm{Ag}(\mathrm{s})+\mathrm{O}_{2}(g)\)

If \(5.76 \mathrm{~g} \text { of } \mathrm{Ag}_{2} \mathrm{O}\) is heated and the \(\mathrm{O}_{2}\) gas produced by the reaction is collected in an evacuated flask, what is the pressure of the \(\mathrm{O}_{2}\) gas if the volume of the flask is \(0.65 \mathrm{~L}\) and the gas temperature is \(25^{\circ} \mathrm{C}\)?

 

(a)  \(0.94 \mathrm{~atm}\)

(b) \(0.039 \mathrm{~atm}\)

(c) \(0.012 \mathrm{~atm}\)

(d)  \(0.47 \mathrm{~atm}\)

(e)  \(3.2 \mathrm{~atm}\)

Equation Transcription:

Text Transcription:

2Ag2O(s) \rightarrow^{\Delta} 4Ag(s)+O2(g)

5.76  g  of  Ag2O

O2

O2

0.65 L

25°C

0.94 atm

0.039 atm

0.012 atm

0.47 atm

3.2 atm