What volume of carbon dioxide gas is produced at NTP when 20gram of 20percent pure caco3 is completely heated
How much CaCO3 do you have? That's 20 g x (1.00 - 0.20) = 16
CaCO3 ==> CaO + CO2
mols CaCO3 = 16/molar mass CaCO3 = ?
mols CaCO3 = mols CO2 from the equation.
mols CO2 x 24 L/mol @ NTP.
OR you can use 22.4 L/mol @ STP and convert to NTP by correcting for the T from 273.15K to 293.15 K. I have estimated the 24 number above.
Post your work if you get stuck.
To find the volume of carbon dioxide gas produced at NTP (Normal Temperature and Pressure) when 20 grams of 20% pure CaCO3 is completely heated, we need to follow a few steps:
1. Calculate the number of moles of CaCO3:
- Convert the mass of CaCO3 to moles using its molar mass. The molar mass of CaCO3 is:
- (1 x molar mass of Ca) + (1 x molar mass of C) + (3 x molar mass of O)
- Approximate molar mass of CaCO3 = 40 g/mol + 12 g/mol + (3 x 16 g/mol) = 100 g/mol
- Moles = mass / molar mass
- Moles of CaCO3 = 20 g / 100 g/mol = 0.2 moles
2. Calculate the moles of CO2 produced:
- Since CaCO3 decomposes into CaO and CO2, the balanced equation for the reaction is:
CaCO3 -> CaO + CO2
- According to the equation, 1 mole of CaCO3 produces 1 mole of CO2.
- Therefore, moles of CO2 = moles of CaCO3 = 0.2 moles
3. Calculate the volume of CO2 gas at NTP:
- At NTP, the conditions are usually defined as a temperature of 0 degrees Celsius (273.15 Kelvin) and a pressure of 1 atmosphere (101.325 kPa).
- The ideal gas law, PV = nRT, can be used to find the volume of the gas.
- Rearranging the equation, V = nRT / P, where V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), T is the temperature in Kelvin, and P is the pressure.
- Plugging in the values:
V = (0.2 moles) x (0.0821 L·atm/(mol·K)) x (273.15 K) / (1 atm)
- Calculating this expression will give the volume of CO2 gas produced at NTP.
By following these steps, you should be able to calculate the volume of carbon dioxide gas produced at NTP when 20 grams of 20% pure CaCO3 is completely heated.