Answer:
To determine the number of liters of carbon dioxide at STP (Standard Temperature and Pressure) given the mass of 22.87 grams, we need to use the concept of molar mass and the ideal gas law.
First, we need to find the number of moles of carbon dioxide. We can do this by dividing the mass of carbon dioxide by its molar mass. The molar mass of carbon dioxide (CO2) is approximately 44.01 grams/mol.
Number of moles of carbon dioxide = mass of carbon dioxide / molar mass of carbon dioxide
Number of moles of carbon dioxide = 22.87 g / 44.01 g/mol
Next, we can use the ideal gas law, which states that at STP, one mole of any ideal gas occupies a volume of 22.4 liters. So, the number of liters of carbon dioxide at STP will be equal to the number of moles of carbon dioxide multiplied by 22.4 liters/mol.
Number of liters of carbon dioxide at STP = number of moles of carbon dioxide * 22.4 liters/mol
Substituting the value we obtained for the number of moles of carbon dioxide:
Number of liters of carbon dioxide at STP = (22.87 g / 44.01 g/mol) * 22.4 liters/mol
Calculating this expression will give us the final answer.
Please note that you have provided the mass of carbon dioxide, but not the volume or pressure at which the gas is measured. Therefore, we assumed STP conditions for this calculation.