CH4 + 20 2 --> CO2 + 2H2O
How many liters of CO2 would be produced if 32 grams of CH4 are combined with oxygen???
How many grams of H2O would be produced when the 32 grams of CH4 are burned???
To find the number of liters of CO2 produced when 32 grams of CH4 are combined with oxygen, we need to follow these steps:
Step 1: Convert grams of CH4 to moles of CH4:
To do this, we need to know the molar mass of CH4 (methane). Since the molar mass of carbon (C) is 12.01 g/mol and the molar mass of hydrogen (H) is 1.008 g/mol, we calculate the molar mass of CH4 as follows:
Molar mass of CH4 = (1 × molar mass of C) + (4 × molar mass of H)
= (1 × 12.01 g/mol) + (4 × 1.008 g/mol)
= 12.01 g/mol + 4.032 g/mol
= 16.042 g/mol
Now, we can convert grams of CH4 to moles by using the following formula:
moles of CH4 = (mass of CH4) / (molar mass of CH4)
= 32 g / 16.042 g/mol
= 1.9939 mol (rounded to 4 decimal places)
Step 2: Use stoichiometry to determine the moles of CO2 produced:
From the balanced chemical equation, we can see that the stoichiometric ratio between CH4 and CO2 is 1:1. Therefore, the number of moles of CO2 produced will also be 1.9939 mol.
Step 3: Convert moles of CO2 to liters of CO2:
To convert moles to liters, we need to use the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L⋅atm / K⋅mol), and T is the temperature in Kelvin.
Since the volume and pressure are not provided in the question, we can assume that the reaction is taking place at standard temperature and pressure (STP).
At STP, the temperature is 273.15 K, and the pressure is 1 atm.
Using the ideal gas law equation, we can rearrange it to solve for V (volume):
V = (nRT) / P
Substituting the values, we get:
V = (1.9939 mol) × (0.0821 L⋅atm / K⋅mol) × (273.15 K) / (1 atm)
≈ 45.7 L (rounded to 2 decimal places)
Therefore, approximately 45.7 liters of CO2 would be produced when 32 grams of CH4 are combined with oxygen.
To find the number of grams of H2O produced when 32 grams of CH4 are burned, we use the same approach:
Step 1: Convert grams of CH4 to moles of CH4:
We have already calculated this in the previous question, which is 1.9939 moles.
Step 2: Use stoichiometry to determine the moles of H2O produced:
From the balanced chemical equation, we can see that the stoichiometric ratio between CH4 and H2O is 1:2. Therefore, the number of moles of H2O produced will be 2 × 1.9939 mol = 3.9878 mol (rounded to 4 decimal places).
Step 3: Convert moles of H2O to grams of H2O:
To convert moles to grams, we need to use the molar mass of H2O. The molar mass of water (H2O) is 18.015 g/mol.
Using the formula:
mass of H2O = (moles of H2O) × (molar mass of H2O)
= 3.9878 mol × 18.015 g/mol
≈ 71.8 g (rounded to 1 decimal place)
Therefore, approximately 71.8 grams of H2O would be produced when 32 grams of CH4 are burned.