In the reaction shown here, $4\mathrm{.}90L$ of $O_2$ was formed at $P=734mmHg$ and $T=308$

$K.$

$2A{g}_{2}O(s)4Ag(s)+O_2(g)$

You may want to reference $($Pages $444-446)$ Section $10\mathrm{.}10$ while completing this

problem.

Part A

How many grams of $A{g}_{2}O$ decomposed?

Express the mass to three significant figures and include the appropriate

units.

Previous Answers

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Use the ideal gas equation $(PV=nRT)$ to calculate the number of

moles of gas $(O_2)$ based on the given volume $($in $L),$ pressure $($in atm$),$

and temperature $($in $K).$ Then, use a stoichiometric conversion factor

$($derived from the balanced chemical equation$)$ to determine the moles of

$A{g}_{2}O$ that reacted. Lastly, use the molar mass of

$\frac{g}{m}ol)$ to calculate the corresponding mass in grams.