Question

In the following reaction, 4.58 L of O₂ was formed at P = 745 mmHg and T = 308 K. How many grams of Ag₂O decomposed?

2 Ag₂O → 4 Ag + O₂
A) 3.25 g
B) 6.50 g
C) 9.75 g
D) 13.00 g

Answer 1

The correct answer is D) 13.00 g.

Step-by-step explanation:

The given reaction is:

2 Ag₂O → 4 Ag + O₂

From the balanced equation, we can see that 2 moles of Ag₂O decompose to form 4 moles of Ag and 1 mole of O₂.

We are given that 4.58 L of O₂ was formed at P = 745 mmHg and T = 308 K.

Using the ideal gas law, we can calculate the number of moles of O₂ using the given volume, pressure, and temperature.

Then, based on the stoichiometry of the reaction, we can determine the moles of Ag₂O decomposed.

Finally, we can convert the moles of Ag₂O to grams using the molar mass of Ag₂O.

The correct answer is D) 13.00 g.