Question

When the amount of oxygen is limited, carbon and oxygen react to form carbon monoxide. How many grams of CO can be formed from 35 grams of oxygen? 2C + O2 → 2CO What is the molecular mass of oxygen? g/mole What is the molecular mass of carbon monoxide?

Answer 1

Approximately 61.27 grams of CO can be formed from 35 grams of oxygen.

The molecular mass of oxygen (O2) is 32 g/mol, and the molecular mass of carbon monoxide (CO) is 28.01 g/mol.

The balanced chemical equation for the reaction is:

2C + O2 → 2CO.

From the balanced equation, we can see that 1 mole of O2 reacts to form 2 moles of CO. Therefore, the number of moles of O2 in 35 grams is:

`$\frac{35 \text{ g}}{32 \text{ g/mol}} = 1.09375 \text{ moles}$$`

Since 1 mole of O2 forms 2 moles of CO, the number of moles of CO formed is:

`$$1.09375 \text{ moles} * 2 = 2.1875 \text{ moles}$$`

Therefore, the mass of CO formed is:

`$$2.1875 \text{ moles} * 28.01 \text{ g/mol} = 61.27 \text{ g}$$`

So, approximately 61.27 grams of CO can be formed from 35 grams of oxygen.

Answer 2

(a) 61.25g

(b) 32g/mol

(c) 28g/mol

Step-by-step explanation:

From the equation of reaction, we can see that 1 mole of oxygen yielded 2 moles of CO.

Now to the number of grams of CO question, we first need to calculate the number of moles of oxygen reacted.

The number of moles equal the mass of oxygen reacted divided by the molar mass of oxygen.

The molecular mass of oxygen molecule is 2(16) which equals 32g/mol ( 16 is the atomic mass unit of the oxygen atom and the oxygen molecule has 2 atoms)

Now, the number of moles of oxygen reacted is 35/32 moles.

If 1 mole of oxygen yielded 2 moles of carbon ii oxide, 35/32 moles will yield 35/32 × 2 which equals 35/16 moles.

From here, we can calculate the mass of CO yielded. That equals the number of moles of CO yielded multiplied by the molar mass of CO.

The molar mass of CO is 12 + 16 = 28g/mol ( the atomic mass of carbon is 12 a.m.u)

Now we divide 35/16 × 28

This equals 61.25g