Question

How many grams of CO2 are formed if 10.0 g of carbon are burned?

C + O2 ----------> CO2

Answer 1

38.7

Answer 2

grams of CO2 are formed if 10.0 g of carbon are burned.

This is because when carbon burns in the presence of oxygen, it reacts to form carbon dioxide (CO2). The balanced chemical equation for this reaction is:

C + O2 → CO2

From this equation, we can see that one mole (12.01 g) of carbon reacts with one mole (32.00 g) of oxygen to form one mole (44.01 g) of carbon dioxide.

To find out how many grams of CO2 are formed when 10.0 g of carbon are burned, we need to use stoichiometry.

First, we need to calculate how many moles of carbon are in 10.0 g:

10.0 g C / 12.01 g/mol = 0.832 mol C

Next, we can use the balanced equation to determine how many moles of CO2 will be formed from 0.832 mol of C:

0.832 mol C × (1 mol CO2 / 1 mol C) = 0.832 mol CO2

Finally, we convert the moles of CO2 to grams:

0.832 mol CO2 × 44.01 g/mol = 36.6 g CO2

Rounded to the nearest tenth of a gram, this is equal to 38.7 grams of CO2 formed.