With the combustion of methane, CH4, If 150 Liters of carbon dioxide are produced, how many grams of methane required?
CH4+2O2>> CO2 + 2H2O
law of volumes applies..then if 150 liters carbon dioxide, one got then also 300 liters of water vapor, and used 150 liters of methane...
Now, grams of methane...At what temperature did all this occur, and pressure?
In order to find the number of grams of methane required, we need to calculate the molar ratio between methane (CH4) and carbon dioxide (CO2). This can be achieved by using the balanced chemical equation for the combustion of methane:
CH4 + 2O2 -> CO2 + 2H2O
From the equation, it is clear that for every methane molecule (CH4) combusted, one molecule of carbon dioxide (CO2) is produced.
To determine the number of moles of carbon dioxide produced, we will use the ideal gas law equation, which states that:
PV = nRT
Where:
P = pressure (in atmospheres),
V = volume (in liters),
n = number of moles,
R = ideal gas constant (0.0821 L∙atm/(mol∙K)),
T = temperature (in Kelvin).
In this specific case, we are given the volume of carbon dioxide produced, which is 150 liters. Since we are dealing with gases, we also have to consider the temperature and pressure. Assuming the temperature and pressure are constant, we can simplify the equation to:
V = nRT
Now, we can solve for the number of moles of carbon dioxide (n). Substituting the given values:
150 L = n * (0.0821 L∙atm/(mol∙K)) * T
Since we are calculating the number of moles of carbon dioxide, we can use this equation to find the number of moles of methane required as well.
Based on the balanced chemical equation, the molar ratio between CH4 and CO2 is 1:1. This means that the number of moles of methane required is equal to the number of moles of carbon dioxide produced.
Therefore, if 150 liters of carbon dioxide are produced, the number of moles of methane required is also 150 moles.
To convert moles to grams, we need to know the molar mass of methane (CH4). The molar mass of carbon (C) is 12.01 g/mol, and the molar mass of hydrogen (H) is 1.01 g/mol. Adding these together, we get:
(12.01 g/mol) + 4(1.01 g/mol) = 16.05 g/mol
Thus, the molar mass of methane is 16.05 g/mol.
To calculate the mass of methane, we multiply the number of moles (150) by the molar mass (16.05 g/mol):
Mass of methane = 150 moles * 16.05 g/mol
Therefore, the mass of methane required is 2407.5 grams.