To calculate the volume of CO2 produced by the decomposition of CuCO3•Cu(OH)2 at STP, you need to follow a step-by-step approach. Here's how you can do it:
Step 1: Write the balanced equation for the reaction:
CuCO3•Cu(OH)2(s) -> CuO(s) + CO2(g) + H2O(g)
Step 2: Determine the molar mass of CuCO3•Cu(OH)2:
CuCO3•Cu(OH)2 = CuCO3 + Cu(OH)2
CuCO3: Cu (atomic mass = 63.546 g/mol) + C (12.01 g/mol) + 3 O (16.00 g/mol) = 123.546 g/mol
Cu(OH)2: Cu (atomic mass = 63.546 g/mol) + 2 O (16.00 g/mol) + 2 H (1.01 g/mol) = 99.546 g/mol
The molar mass of CuCO3•Cu(OH)2 = 123.546 g/mol + 99.546 g/mol = 223.092 g/mol
Step 3: Calculate the number of moles of CuCO3•Cu(OH)2:
moles = mass / molar mass
moles = 2.21 g / 223.092 g/mol = 0.0099 mol
Step 4: Use the balanced equation to determine the mole ratio of CO2 to CuCO3•Cu(OH)2:
From the balanced equation, the mole ratio is 1:1. This means that for every 1 mole of CuCO3•Cu(OH)2, 1 mole of CO2 is produced.
Step 5: Calculate the volume of CO2 at STP:
1 mole of any ideal gas occupies 22.4 L at standard temperature and pressure (STP).
volume = moles x 22.4 L/mol
volume = 0.0099 mol x 22.4 L/mol = 0.22176 L
Therefore, the volume of CO2 produced by the decomposition of 2.21 g of CuCO3•Cu(OH)2 at STP is approximately 0.22176 liters.