what mass of carbon, in grams, can be consumed by 44 g oxygen in in combustion to give carbon monoxide/ what mass of CO is produced?

To determine the mass of carbon that can be consumed by 44 g of oxygen in combustion, we need to use the balanced chemical equation for the combustion of carbon.

The balanced equation for the combustion of carbon is:
C + O2 → CO2

From the equation, we can see that 1 mole of carbon reacts with 1 mole of oxygen to produce 1 mole of carbon dioxide.

Next, we need to find the molar mass of carbon dioxide, which is 44 g/mol.

Using the molar mass ratio between oxygen and carbon dioxide, we can calculate the amount of oxygen required to produce 44 g of carbon dioxide.

Molar mass of oxygen (O2) = 32 g/mol
Molar mass of carbon dioxide (CO2) = 44 g/mol

Mass of carbon dioxide produced = 44 g

Now, we can set up a ratio based on the ratio of oxygen and carbon dioxide:

(32 g O2 / 44 g CO2) = (44 g O2 / x)

Solving for x, we get:

x = (44 g CO2 * 32 g O2) / 44 g O2
x = 32 g CO2

Therefore, the mass of carbon consumed by 44 g of oxygen in combustion is equal to the mass of carbon dioxide produced, which is 32 grams.

Let's move on to calculate the mass of carbon monoxide produced.

To find the mass of carbon monoxide produced, we need to know the balanced chemical equation for the combustion of carbon to carbon monoxide.

The balanced equation for the combustion of carbon to carbon monoxide is:
2C + O2 → 2CO

From this equation, we can see that 2 moles of carbon react with 1 mole of oxygen to produce 2 moles of carbon monoxide.

Using the molar mass of carbon monoxide, which is 28 g/mol, we can determine the mass of carbon monoxide produced.

Molar mass of carbon monoxide (CO) = 28 g/mol

Using the molar mass ratio between oxygen and carbon monoxide, we can calculate the mass of carbon monoxide produced.

(32 g O2 / 2(28 g CO)) = (44 g O2 / x)

Solving for x, we get:

x = (44 g O2 * 2(28 g CO)) / 32 g O2
x = 77 g CO

Therefore, the mass of carbon monoxide produced is 77 grams.