How many liters of CO2 would be produced if 32 grams of CH4 are combined with oxygen?
balance the equation
methane+oxygen>>carbon dioxide + water.
then, how many moles of methane is in 32 grams?
Then, use the mole ratio on the balanced equation coefficents to answer the questions.
To determine the number of liters of CO2 produced when 32 grams of CH4 are combined with oxygen, you need to follow these steps:
Step 1: Write the balanced equation for the combustion of methane (CH4).
CH4 + 2O2 → CO2 + 2H2O
Step 2: Calculate the molar mass of CH4.
Molar mass of carbon (C) = 12.01 g/mol
Molar mass of hydrogen (H) = 1.008 g/mol
Molar mass of CH4 = (12.01 g/mol) + 4 * (1.008 g/mol) = 16.04 g/mol
Step 3: Convert the given mass of CH4 to moles.
Moles of CH4 = (32 g) / (16.04 g/mol) = 1.994 mol (rounded to three decimal places)
Step 4: Determine the moles of CO2 produced using the stoichiometry of the balanced equation.
From the balanced equation, you can see that for every 1 mol of CH4, 1 mol of CO2 is produced. Therefore, the moles of CO2 produced are also 1.994 mol.
Step 5: Convert the moles of CO2 to volume using the ideal gas law.
The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is temperature in Kelvin.
Assuming the conditions are at standard temperature and pressure (STP), where temperature is 273.15 K and pressure is 1 atm, the ideal gas law can be simplified to V = n * 22.4 L/mol.
The volume of CO2 = (1.994 mol) * (22.4 L/mol) = 44.2616 L (rounded to four decimal places)
Therefore, when 32 grams of CH4 are combined with oxygen, approximately 44.2616 liters of CO2 would be produced.