When carbon is burned in air, it reacts with oxygen to form carbon dioxide. when 13.2 g of carbon were burned in the presence of 53.9 g of oxygen 18.7 g of oxygen remained unredacted. what mass of carbon dioxide was produced?

grams of CO2 produced = 48.4 grams

Explanation:

Write the balance equation of the reaction . The chemical equation is represented below

C(s) + O2(g) → CO2(g)

The equation is already balanced.  From the reaction carbon is the limiting reagent and it is use in the computation of mass for the product . Oxygen is in excess.

C(s) + O2(g) → CO2(g)

atomic mass of carbon = 12 g/mol

atomic mass of oxygen = 16 g/mol

Molar mass of carbon dioxide =  12 + 16(2) = 12 + 32 = 44 grams

if 12 g of C produce 44 grams of CO2

13.2 grams of C will produce ? grams of CO2

cross multiply

grams of CO2 produced = (13.2 × 44)/12

grams of CO2 produced = 580.8/12

grams of CO2 produced = 48.4 grams

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !