How many Lister of Carbon Dioxide gas measured at STP can be produced by the decomposition of 15.0g of Sodium Bicarbonate to give Sodium Carbonate, water, and Carbon Dioxide gas?
Here is a worked example of a simple stoichiometry problem.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine how many liters of carbon dioxide gas can be produced by the decomposition of sodium bicarbonate, we need to follow a series of steps. Let's break it down:
Step 1: Write the balanced chemical equation for the decomposition reaction of sodium bicarbonate (NaHCO3):
2 NaHCO3(s) -> Na2CO3(s) + H2O(g) + CO2(g)
From the balanced equation, we can see that 2 moles of sodium bicarbonate produce 1 mole of carbon dioxide gas.
Step 2: Calculate the molar mass of sodium bicarbonate (NaHCO3):
Na = 22.99 g/mol
H = 1.01 g/mol
C = 12.01 g/mol
O = 16.00 g/mol
Molar mass of NaHCO3:
(22.99 g/mol) + (1.01 g/mol) + (12.01 g/mol) + (3 * 16.00 g/mol) = 84.01 g/mol
Step 3: Calculate the number of moles of sodium bicarbonate (NaHCO3):
Given mass of sodium bicarbonate = 15.0 g
Number of moles = (mass of substance) / (molar mass)
Number of moles = (15.0 g) / (84.01 g/mol)
Step 4: Determine the number of moles of carbon dioxide (CO2) produced:
From the balanced equation, we know that 2 moles of NaHCO3 produce 1 mole of CO2.
This means the number of moles of CO2 is half the number of moles of NaHCO3.
Moles of CO2 = (0.5) * (number of moles of NaHCO3)
Step 5: Use the ideal gas law to convert moles of CO2 to volume (liters) at standard temperature and pressure (STP):
At STP, the conditions are 1 atmosphere (atm) of pressure and 273.15 K (0 degrees Celsius) of temperature. Also, the molar volume of any gas at STP is approximately 22.4 L/mol.
Volume (liters) of CO2 = (number of moles of CO2) * (molar volume at STP)
Now, you can plug in the values and calculate the result.