CO + 2*H2 --> CH3OH
How many moles of each reactant are needed to produce 3.60 x 10^2g CH3OH?
I appreciate anyone who helps me with this. Also, please say the steps on how you got your answer.
Balance the equation. I think it is balanced.
Convert 360 g CH3OH to mols CH3OH.
mols = g/molar mass CH3OH.
Use the coefficients in the balanced equation to convert mols CH3OH to mols CO and do a separate one to convert to mols H2.
Post your work if you get stuck but explain what you don't understand.
To balance the equation, it is already balanced:
CO + 2H2 → CH3OH
To convert 360 g CH3OH to mols CH3OH, use the molar mass of CH3OH:
mols CH3OH = 360 g CH3OH / 32.04 g/mol CH3OH = 11.25 mols CH3OH
To convert mols CH3OH to mols CO and mols H2, use the coefficients in the balanced equation:
mols CO = 11.25 mols CH3OH / 1 mol CO = 11.25 mols CO
mols H2 = 11.25 mols CH3OH / 2 mols H2 = 5.625 mols H2
Therefore, 11.25 mols CO and 5.625 mols H2 are needed to produce 360 g CH3OH.
To determine how many moles of each reactant are needed to produce 3.60 x 10^2 g of CH3OH, follow these steps:
1. Balance the equation: CO + 2H2 → CH3OH
The equation is already balanced, so we can proceed to the next step.
2. Convert 360 g of CH3OH to moles of CH3OH.
To do this, we need the molar mass of CH3OH, which is the sum of the atomic masses of all the atoms in one molecule of CH3OH:
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.008 g/mol
Molar mass of O = 16.00 g/mol
Molar mass of CH3OH = (12.01 + 1.008 + 1.008 + 1.008 + 16.00) g/mol = 32.04 g/mol
Now we can calculate the number of moles of CH3OH:
moles CH3OH = mass CH3OH / molar mass CH3OH
moles CH3OH = 360 g / 32.04 g/mol = 11.236 mol
So, we have 11.236 moles of CH3OH.
3. Use the coefficients in the balanced equation to convert from moles of CH3OH to moles of CO and H2.
From the balanced equation, we can see that the coefficient of CO is 1, and the coefficient of H2 is 2.
moles CO = moles CH3OH x (coeff. of CO / coeff. of CH3OH)
moles CO = 11.236 mol x (1 / 1) = 11.236 mol
moles H2 = moles CH3OH x (coeff. of H2 / coeff. of CH3OH)
moles H2 = 11.236 mol x (2 / 1) = 22.472 mol
Therefore, to produce 3.60 x 10^2 g of CH3OH, you would need 11.236 moles of CO and 22.472 moles of H2.
To determine the number of moles of each reactant needed to produce 3.60 x 10^2g of CH3OH, let's follow the steps you provided:
Step 1: Balance the equation
The given equation CO + 2H2 -> CH3OH is already balanced.
Step 2: Convert 360g CH3OH to moles CH3OH
To do this, divide the given mass by the molar mass of CH3OH:
molar mass CH3OH = (12.01g/mol x 1) + (1.01g/mol x 4) + (16.00g/mol + 1) = 32.04g/mol
mols CH3OH = 360g / 32.04g/mol ≈ 11.24 mol CH3OH
Step 3: Use the coefficients in the balanced equation to convert moles of CH3OH to moles of CO and H2
From the balanced equation CO + 2H2 -> CH3OH, we see that:
1 mol CO is required for every 1 mol CH3OH
2 mol H2 is required for every 1 mol CH3OH
So, we can conclude that:
11.24 mol CH3OH = 11.24 mol CO (since the coefficient of CO is 1)
11.24 mol CH3OH = 2 * 11.24 mol H2 (since the coefficient of H2 is 2)
Therefore, you would need 11.24 moles of CO and 22.48 moles of H2 to produce 3.60 x 10^2g of CH3OH.