Using the balanced equation for this reaction, calculate the volume of CO2 that should be produced by the decomposition of 2.21g of CuCO3•Cu(OH)2 at STP.
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.