Silver chloride decomposes in light to produce silver and chlorine.
What mass of silver is produced when 25g of silver chloride completely decomposes?
What volume of chlorine is produced at STP?
Follow the steps in this example.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Thank you soo muchh (:
To find the mass of silver produced, you need to use the balanced chemical equation for the decomposition of silver chloride. The balanced equation is:
2 AgCl(s) → 2 Ag(s) + Cl2(g)
From the equation, you can see that 2 moles of silver chloride (AgCl) produce 2 moles of silver (Ag). The molar mass of silver is 107.87 g/mol.
To find the moles of silver chloride, divide the given mass (25g) by its molar mass (143.32 g/mol):
Moles of AgCl = Mass of AgCl / Molar mass of AgCl
Moles of AgCl = 25g / 143.32 g/mol ≈ 0.1746 mol
Now, since the ratio of AgCl to Ag is 1:1, the moles of silver produced will be the same as the moles of silver chloride. So, the moles of silver (Ag) produced are also 0.1746 mol.
To get the mass of silver (Ag), multiply the moles of silver by its molar mass:
Mass of Ag = Moles of Ag x Molar mass of Ag
Mass of Ag = 0.1746 mol x 107.87 g/mol ≈ 18.82 g
Therefore, approximately 18.82 grams of silver will be produced when 25 grams of silver chloride completely decomposes.
Now, let's find the volume of chlorine produced at STP (Standard Temperature and Pressure). According to the balanced equation, 1 mole of silver chloride produces 1 mole of chlorine gas (Cl2).
At STP, 1 mole of gas occupies 22.4 liters. So, to find the volume of chlorine gas produced, you need to convert moles of chlorine gas to liters.
Moles of Cl2 = Moles of AgCl = 0.1746 mol
Volume of Cl2 = Moles of Cl2 x Molar volume at STP
Volume of Cl2 = 0.1746 mol x 22.4 L/mol ≈ 3.91 L
Therefore, approximately 3.91 liters of chlorine gas will be produced at STP when 25 grams of silver chloride completely decomposes.