If 6.0g of CH4 and 5.0g of O2 are used, what is the mass of CO2 produced?
Step 1:Write the chemical equation of the oxidation:
CH4+2O2=CO2+2H2O
This means that 1 mole of CH4 or 2 moles of O2 will give 1 mole of CO2
Step 2: find limiting reagent
CH4: 6/(12+4*1)=6/16=0.4375 mol
O2: 5/(2*16)=5/32=0.15625 mol
Compare with the equation in step 1, it is evident that O2 is the limiting reagent.
Step 3: find quantity of CO2 produced by the limiting reagent.
From chemical equation, we know that 2 mol of O2 will produce 1 mol of CO2.
By proportion,
0.15625 mol of O2 will produce 0.15625/2 mol=0.78125 of CO2.
Find the mass of 0.78125 mol of CO2, round answer to 2 significant figures.
To calculate the mass of CO2 produced when 6.0g of CH4 (methane) and 5.0g of O2 (oxygen) react, we need to balance the chemical equation and calculate the molar masses.
Step 1: Write and balance the chemical equation.
The balanced equation for the reaction between CH4 and O2 to produce CO2 is:
CH4 + 2O2 → CO2 + 2H2O
Step 2: Calculate the molar masses.
Using the periodic table, we can find the molar masses of the elements involved:
- Molar mass of CH4 (methane): 12.01g (C) + 4(1.01g) (4H) = 16.05g/mol
- Molar mass of O2 (oxygen): 16.00g/mol (since O2 is a diatomic molecule)
- Molar mass of CO2 (carbon dioxide): 12.01g (C) + 2(16.00g) (2O) = 44.01g/mol
Step 3: Calculate the moles of each substance.
To find the moles of each substance, divide the given mass by its molar mass:
- Moles of CH4 = 6.0g / 16.05g/mol = 0.37 mol
- Moles of O2 = 5.0g / 32.00g/mol = 0.16 mol
Step 4: Use the balanced equation to determine the stoichiometry.
From the balanced equation, we can see that:
- 1 mole of CH4 reacts with 2 moles of O2 to produce 1 mole of CO2.
- This means that 0.37 mol of CH4 will react with 2 * 0.37 mol of O2 to produce 0.37 mol of CO2.
Step 5: Calculate the mass of CO2 produced.
Multiply the moles of CO2 by its molar mass:
Mass of CO2 = 0.37 mol * 44.01g/mol = 16.27g
Therefore, the mass of CO2 produced when 6.0g of CH4 and 5.0g of O2 react is approximately 16.27g.