A 0.600 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g) If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mm Hg at 27°C.

Explanation:

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In this case, for the reaction:

As 13.8 mL (0.0138 L) are collected at 27 °C and 1.00 atm, we can compute the yielded moles of oxygen via the ideal gas equation as shown below, considering that the pressure of oxygen is equal to the total pressure minus the vapor pressure of water (26.7 mmHg=0.035atm):

Next, via the 1:2 mole ratio between oxygen and silver oxide (molar mass = 231.735  g/mol) in the chemical reaction, the mass of pure silver oxide turns out:

In such a way, the percent by mass of silver oxide in the 0.600-g sample is:

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answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.