Calculate the amount of heat required to completely sublime 24.0 g of solid dry ice CO_2 at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.
32.3 kJ/mol x mols CO2 = q (heat required).
How many mols CO2 are in 24.0 g CO2? Something like 24.0/molar mass CO2?
Check my thinking.
To calculate the amount of heat required to sublime 24.0 g of solid dry ice (CO2) at its sublimation temperature, you can follow these steps:
Step 1: Convert the mass of CO2 to moles.
To do this, we'll use the molar mass of CO2, which is 44.01 g/mol.
Moles of CO2 = mass (g) / molar mass (g/mol) = 24.0 g / 44.01 g/mol = 0.5458 mol
Step 2: Calculate the amount of heat required.
The heat of sublimation for carbon dioxide is given as 32.3 kJ/mol.
Heat required = moles of CO2 × heat of sublimation = 0.5458 mol × 32.3 kJ/mol = 17.66434 kJ.
Therefore, the amount of heat required to completely sublime 24.0 g of solid dry ice CO2 at its sublimation temperature is approximately 17.66434 kJ.
To calculate the amount of heat required to completely sublime 24.0 g of solid dry ice (CO2) at its sublimation temperature, we need to follow these steps:
Step 1: Determine the molar mass of CO2
The molar mass of CO2 is calculated by adding the atomic masses of carbon (C) and two oxygen (O) atoms.
C: 12.01 g/mol
O: 16.00 g/mol
Molar mass of CO2 = (12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol
Step 2: Calculate the number of moles of CO2
The number of moles can be calculated using the formula:
moles = mass / molar mass
moles of CO2 = 24.0 g / 44.01 g/mol = 0.545 mol
Step 3: Calculate the amount of heat required
The heat of sublimation for carbon dioxide is given as 32.3 kJ/mol. We can use this value to calculate the heat required to sublime the given amount of CO2.
Amount of heat = moles of CO2 × heat of sublimation
Amount of heat = 0.545 mol × 32.3 kJ/mol = 17.62 kJ
Therefore, the amount of heat required to completely sublime 24.0 g of solid dry ice CO2 at its sublimation temperature is approximately 17.62 kJ.