Consider the unbalanced equation for the decomposition of silver nitrate:
AgNO3(s) ---Ag(s)+NO2(g)+O2(g)

1. Write the balanced equation for the reaction.
2. When 54.0g of AgNO3 is heated, 4.60g of O2 is formed. How many grams of Ag is also formed?

Question

Consider the unbalanced equation for the decomposition of silver nitrate: 
AgNO3(s) --->Ag(s)+NO2(g)+O2(g)
 
1. Write the balanced equation for the reaction.
 2. When 54.0g of AgNO3 is heated, 4.60g of O2 is formed. How many grams of Ag is also formed?

anonymous · Answer

2AgNO3(s) --->2Ag(s)  +  2NO2(g)  +   O2(g) 
Moles of AgNO3:   2 * 4.6/32 = .288 mol
Mass of Ag: .288 * 108 = 31.05 g

anonymous · Answer

can you help me with this please. What is the percent yield of Ag for the reaction?

anonymous · Answer

Theoretical mole of AgNO3: 54/ 170 = .318 mol
Theoretical mass of Ag: .318 * 108 = 34.31g
Percent yield: 31.05 * 100 / 34.31 = 90.51%