Silver oxide (Ag2O) decomposes at temperature 300°C yielding metallic silver and oxygen gas. A 1.60 g sample of impure silver oxide Yields 0.104 g of oxygen gas. What is the percent by mass of the silver oxide in the sample ? - Sri Chaitanya Infinity Learn Best Online Courses for NCERT Solutions, CBSE, ICSE, JEE, NEET, Olympiad and Class 6 to 12

A
5.9
B
47.725
C
94.25
D
88.2

Solution:

Let mass of Ag₂O = x g
$\begin{array}{l} {Ag}_{2} O ⟶ 2 Ag + \frac{1}{2} O_{2} \\ 232 g \frac{1}{2} \times 32 = 16 {gO}_{2} \\ x g 0.104 g of O_{2} \\ One mole of {Ag}_{2} O decompose = \frac{1}{2} mole of O_{2} formed \\ \frac{a}{232} = \frac{1}{2} x \frac{0.104}{32} \\ x = 1 .508 g \\ % g of {Ag}_{2} O = \frac{1 .508}{1 .6} \times 100 = 94 .25 % \end{array}$

Silver oxide (Ag₂O) decomposes at temperature 300°C yielding metallic silver and oxygen gas. A 1.60 g sample of impure silver oxide Yields 0.104 g of oxygen gas. What is the percent by mass of the silver oxide in the sample ?

Solution:

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