In this reaction, 4.58L of #O_2# were formed at 745 mmHg and 308K. How many grams of #Ag_2O# decomposed? #2Ag_2O_((s)) -> 4Ag_((s)) + O_(2(g))#
Your reaction required the decomposition of 82.5 g of silver oxide.
Start with the balanced chemical equation
Notice that you have a
Use the ideal gas law equation to determine how many moles of oxygen were produced
Use the aforementioned mole ratio to determine how many moles of silver oxide reacted
Now use silver oxide's molar mass to determine how many grams would contain this many moles