Hello, I was confused on this chemistry problem and I was wondering if someone could please help me.

1) Consider the following chemical reaction:
2CH3OH(I) + 3O2 (g) → 2CO2(g) + 4H2O(I)

Calculate the number of moles of CO2 produced when 11.25 mL of methanol CH3OH(I) reacted completely with O2(g). The density of methanol is .079 g/mL.

*The density of methanol is 0.79 g/mL

To solve this problem, we need to follow a few steps. Let's break it down:

Step 1: Convert volume of methanol to mass
We are given the volume of methanol as 11.25 mL and the density of methanol as 0.079 g/mL. To find the mass, we can use the formula:
mass = density × volume
mass = 0.079 g/mL × 11.25 mL

Calculating the mass of methanol would give us the starting point to determine the moles.

Step 2: Convert mass of methanol to moles
To convert the mass of methanol to moles, we need the molar mass of methanol (CH3OH). The molar mass can be calculated by adding up the atomic masses of each element present:
C = 12.01 g/mol, H = 1.01 g/mol, O = 16.00 g/mol.

Molar Mass of CH3OH = (12.01 g/mol × 1) + (1.01 g/mol × 4) + (16.00 g/mol × 1) = 32.04 g/mol

Now, we can calculate the number of moles using the formula:
moles = mass / molar mass
moles = (0.079 g/mL × 11.25 mL) / 32.04 g/mol

Step 3: Use stoichiometry to determine the moles of CO2 produced
According to the balanced chemical equation, the stoichiometric ratio between methanol (CH3OH) and CO2 is 2:2. This means that for every 2 moles of methanol reacted, 2 moles of CO2 are produced.

Since we've calculated the number of moles of methanol in step 2, we can conclude that the number of moles of CO2 produced will also be the same.

Final Answer:
The number of moles of CO2 produced when 11.25 mL of methanol reacted completely with O2 is equal to the number of moles of methanol, which is calculated in step 2.

Sure, I can help you with that chemistry problem!

To calculate the number of moles of CO2 produced, we need to follow a few steps:

Step 1: Determine the number of moles of CH3OH reacted.
To do this, we'll use the density of methanol. The density is given as 0.079 g/mL, and we have 11.25 mL of methanol. We can calculate the mass of methanol using the formula:

Mass of methanol (g) = Volume of methanol (mL) × Density of methanol (g/mL)
Mass of methanol (g) = 11.25 mL × 0.079 g/mL

Step 2: Convert the mass of methanol to moles.
To convert grams to moles, we need to know the molar mass of methanol, CH3OH. The molar mass can be found by adding up the atomic masses of carbon (C), hydrogen (H), and oxygen (O).

The atomic masses are:
Carbon (C) = 12.01 g/mol
Hydrogen (H) = 1.01 g/mol
Oxygen (O) = 16.00 g/mol

The molar mass of CH3OH is:
Molar mass of CH3OH = (12.01 g/mol × 1) + (1.01 g/mol × 4) + (16.00 g/mol × 1)

Step 3: Calculate the number of moles of CH3OH.
To calculate the number of moles, we'll divide the mass of methanol by the molar mass of CH3OH.

Number of moles of CH3OH = Mass of CH3OH / Molar mass of CH3OH

Step 4: Use the mole ratio from the balanced equation to calculate the moles of CO2 formed.
From the balanced equation given, we can see that 2 moles of CH3OH reacts to produce 2 moles of CO2.

So, the number of moles of CO2 formed will be equal to the number of moles of CH3OH multiplied by the mole ratio of CO2 to CH3OH.

Number of moles of CO2 = Number of moles of CH3OH × (2 moles of CO2 / 2 moles of CH3OH)

Finally, substitute the values we obtained above into the equation and solve for the number of moles of CO2 produced.

If you had shown your work I could have found the error in half the time it takes to write all of this out.

2CH3OH(I) + 3O2 (g) → 2CO2(g) + 4H2O(I)

mass CH3OH = volume x density
mass CH3OH = 0.79 g/mL x 11.25 mL = ?

mols CH3OH = grams CH3OH/molar mass CH3OH = ?

mols CO2 = mols CH3OH x (2 mols CO2/2 mols CH3OH) = mols CO2 x 2/2 = ?